Creators - KimikApp

Creators / Researchers

Erica S. Cortez

Erica S. Cortez

Hello, I’m Erica S. Cortez, and I’m excited to welcome you to KimikApp, a platform designed to enhance your teaching and learning experience. For teachers, we understand the challenge of making complex topics, like the Mole Concept, engaging and accessible. With KimikApp, we aim to turn that challenge into an opportunity for both you and your students. As Albert Einstein once said, “It is the supreme art of the teacher to awaken joy in creative expression and knowledge.” We hope that KimikApp helps you do just that—ignite curiosity and foster a love of learning in your students. Through interactive resources such as videos, quizzes, and visual aids, KimikApp provides a fresh way to bring Chemistry to life in the classroom, encouraging critical thinking and deeper understanding. Teachers, we’re here to support you in delivering lessons that inspire and engage your students, making Chemistry not only accessible but exciting. For students, whether you're just beginning to explore the Mole Concept or looking to deepen your understanding, KimikApp is designed to make learning Chemistry fun and easy. Remember, as Marie Curie once said, “Nothing in life is to be feared, it is only to be understood.” With KimikApp, you’ll uncover the wonders of Chemistry step by step, at your own pace, and in a way that makes sense to you. The platform offers interactive videos, quizzes, and visual aids that will help you break down complex concepts and build a strong foundation in Chemistry. So, embrace the adventure of learning, ask questions, and dive in—KimikApp is here to guide you every step of the way. Let’s explore the fascinating world of Chemistry together and make each discovery an exciting journey!

Erica S. Cortez is a 22-year-old fourth-year student at Camarines Norte State College, Abano Campus, where she is pursuing a Bachelor of Secondary Education, majoring in Sciences. Growing up in Daet and later attending Basud National High School, Erica’s academic journey has been marked by hard work and passion. She was honored with a Leadership Award in high school and graduated as Salutatorian from Mabini Colleges Inc. in Senior High School. As a recipient of the CHED Scholarship Program and a consistent Dean's Lister, Erica has always strived for excellence. Her curiosity and drive have led her to co-author two research projects: Emitted Carbon Dioxide (CO2) Monitoring Device for Motorcycles (2018) and Solar-Powered Arduino GSM-Based Fire Alarm and Monitoring Device (2021). These projects reflect her deep commitment to using science and technology for practical, sustainable solutions. Beyond academics, Erica’s greatest passion lies in teaching. Her fascination with the natural world fuels her desire to inspire others to explore and appreciate the wonders of science. To her, teaching isn’t just about delivering information; it’s about sparking curiosity, encouraging questions, and guiding students to see the world through a scientific lens. Erica dreams of becoming a science educator who doesn’t just impart knowledge, but also nurtures a love for learning and critical thinking in her students. She believes that education is a powerful tool to shape the future, and through her work, she hopes to inspire the next generation of thinkers and problem solvers to embrace science and its endless possibilities.

Chain D. Habana

Chain D. Habana

Hello, I’m Chain D. Habana, and I’m thrilled to welcome you to KimikApp, your companion for an enriched learning and teaching journey in Chemistry. For teachers, we know that simplifying complex subjects can be challenging. KimikApp is here to transform these challenges into captivating learning moments for you and your students. As Galileo Galilei once noted, “You cannot teach a man anything; you can only help him find it within himself.” KimikApp aims to do just that—ignite curiosity and open doors to understanding through our innovative resources. With tools like interactive videos, quizzes, and visual guides, KimikApp empowers you to create a classroom environment where Chemistry becomes approachable and engaging. For students, whether you're just starting with basic concepts or delving deeper into molecular science, KimikApp makes Chemistry clear and enjoyable. Remember the words of Isaac Newton: “What we know is a drop, what we don’t know is an ocean.” With KimikApp, you’ll dive into the depths of Chemistry, exploring each concept step by step in a way that’s easy to follow. KimikApp is a platform which includes interactive resources, practice quizzes, and visual aids designed to make learning a meaningful experience. Embrace each topic with curiosity, ask questions, and let KimikApp guide you as you uncover the wonders of Chemistry. Let’s explore this exciting journey together and make every discovery unforgettable!

Chain D. Habana is a passionate and dedicated fourth-year student at Camarines Norte State College-Abaño Campus, pursuing a Bachelor of Secondary Education Major in Sciences. At 23, Chain’s commitment to her studies and her chosen field reflects her belief in the transformative power of education. Her academic journey, marked by hard work and resilience, has earned her the Dean's List Award twice, first in 2022 and again in 2024. Chain's devotion to her studies and her drive to excel mirror her commitment to making education a lifelong pursuit. Her goal is to inspire students in the sciences, turning complex subjects into approachable, meaningful learning experiences. Guided by curiosity and a steadfast commitment to her professional growth, Chain continues to make strides in her field, aspiring to positively impact the lives of future learners. Her path towards deciding to become a future educator someday, came from a huge a turn as through her previous years she envisioned herself differently. Back from her Senior High school year, she took the Technical-Vocational Track (TVL) focusing on Culinary Arts and graduated as the valedictorian of class 2019-2020 in St. Francis Caracciolo Culinary Academy Incorporated. Her decision to become a future educator slowly prevailed when she envisioned and asked herself on how she will imagine herself 10 years from now—and that is to be a Licensed Professional Teacher. She personally hold onto her life mantra which is, "Fall down seven times, stand up eight" implying that life comes with impediments and it simply means that no matter how many times you face setbacks or failures, you should always have the resilience and determination to get back up and continue moving forward.

John Paolo Rafer

John Paolo Rafer

"Education is not the filling of a pail, but the lighting of a fire." – William Butler Yeats Hello, I’m John Paolo Rafer, and I’m thrilled to welcome you to KimikApp, a platform designed to make Chemistry more accessible and exciting. For teachers, we know that explaining the Mole Concept can be challenging—it’s foundational yet complex. With KimikApp, we’re here to support you in transforming this essential topic into an engaging learning experience. Using interactive videos, visual aids, and quizzes, KimikApp brings the Mole Concept to life, helping you inspire curiosity and deepen understanding in your students. For students, whether you're just starting to learn about the Mole Concept or wanting to solidify your knowledge, KimikApp is here to guide you every step of the way. Remember, as Marie Curie once said, “Nothing in life is to be feared; it is only to be understood.” With our resources, you’ll gain confidence in mastering this core Chemistry topic at your own pace. So, dive into the world of Chemistry with KimikApp—explore, understand, and make each discovery an exciting step in your learning journey!

John Paolo Rafer, 21 years old, born on November 21, 2002. Currently in 4th Year of studying at Camarines Norte State College -- College of Education - Abaño Campus with a degree program of Bachelor of Secondary Education Major in Sciences. Scholar of Depart of Science and Technology (R.A. 7687) and Scholar also of Vinzons Municipality. Graduated elementary at Sto. Domingo Vinzons Camarines Norte, Junior High school at D.Q. Liwag National High School, Senior High School at St. Francis Caracciolo Culinary Academy (ABM strand), awarded Best in Science for Batch 2021. Authored two research studies, one about Bad Debt Effects to Small and Medium Business Enterprises (2021). Bacame a News Writer at Caracciolo’s Scribe school’s publication and participated in Division’s Press Conference. He also became Debate adjudicator for GEC 4 - Debate Competition conducted at CNSC - Abaño Campus (May,2023). John Paolo Rafer’s academic journey is marked by a strong dedication to learning and a commitment to excellence, especially within the field of science education. Recognized as a Dean’s Lister for three consecutive years, John Paolo is dedicated to transforming complex scientific concepts into meaningful learning experiences that inspire curiosity and deepen understanding among future students. Interestingly, John’s path to education took an unexpected turn. In senior high school, he initially followed the ABM strand at St. Francis Caracciolo Culinary Academy, focusing on a potential career in business. Yet, as he reflected on his long-term goals, he realized his passion for teaching and envisioned himself making a positive impact in educating. With a desire to bring science to life for students, he shifted his focus toward education, aiming to make a difference in students' lives by inspiring a love for science.

 REFERENCES

Admin. (2023, May 25). Percentage Composition Formula & Solved Examples | Byju’s. BYJUS. https://byjus.com/percent-composition-formula/

Admin. (2023, May 29). Chemistry - Introduction, Branches, Concepts, History & Facts with Free Resources. BYJUS. https://byjus.com/chemistry/

Ball, D. W., & Key, J. A. (2014, September 16). The Mole. Pressbooks. https://opentextbc.ca/introductorychemistry/chapter/the-mole/

Ball, J. a. K. a. D. W. (n.d.). 7.1 The Mole Concept | Introductory Chemistry. https://courses.lumenlearning.com/suny-mcc-introductorychemistry/chapter/formula-mass-and-mole-concept-from-che100/#:~:text=A%20convenient%20amount%20unit%20for,substance%20is%20its%20molar%20mass.

CK-12 Foundation. Mole Carnival. CK-12 Foundation, n.d. https://interactives.ck12.org/simulations/chemistry/mole-carnival/app/index.html

Department of Education, Republic of the Philippines. (2014). Science learner's module 9. Department of Education.

Grade 9 Science Book. (n.d.). DepEd. https://docs.google.com/file/d/0B_TibwEltyeuclc3eVplemVUN0E/preview?resourcekey=0-cu6ZUFhSzCC4WMdiA2OCdg

Helmenstine, A. (2021, May 2). Electronegativity Definition and Trend. Science Notes and Projects. https://sciencenotes.org/electronegativity-definition-and-trend/

Helmenstine, A. M., PhD. (2024, August 2). How to calculate mass percent Composition. ThoughtCo. https://www.thoughtco.com/mass-percent-composition-example-609567

Iwant2study.org (2015) Reading Scale Simulator https://iwant2study.org/lookangejss/math/ejss_model_SHMmassscale/SHMmassscale_Simulation.xhtml

Libretexts. (2011) 2.9: Determining the Mass, Moles, and Number of Particles. Chemistry Libretexts.https://chem.libretexts.org/Courses/University_of_Arkansas_Little_Rock/Chem_1402%3A_General_Chemistry_1_(Kattoum)/Text/2%3A_Atoms%2C_Molecules%2C_and_Ions/2.09%3A_Molecules%2C_Compounds%2C_and_the_Mole

Libretexts. (2021, December 26). 2.10: percent composition. Chemistry LibreTexts. https://chem.libretexts.org/Courses/University_of_Arkansas_Little_Rock/Chem_1402%3A_General_Chemistry_1_(Kattoum)/Text/2%3A_Atoms%2C_Molecules%2C_and_Ions/5.13%3A_Percent_Composition

Libretexts. (2022, July 28). 10.3: Mole-to-Mass, Mass-to-Mole, and Mass-to-Mass conversions. Chemistry LibreTexts. https://chem.libretexts.org/Courses/Portland_Community_College/CH151%3A_Preparatory_Chemistry/10%3A_Mass_Relations_in_Chemical_Reactions/10.03%3A_Mole-to-Mass_Mass-to-Mole_and_Mass-to-Mass_Conversions

Libretexts. (2023, August 9). 5.1: The Law of Conservation of Matter  Chemistry LibreTexts. https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Basics_of_General_Organic_and_Biological_Chemistry_(Ball_et_al.)/05%3A_Introduction_to_Chemical_Reactions/5.01%3A_The_Law_of_Conservation_of_Matter

Percent composition | Formula & calculation - lesson | Study.com. (n.d.). study.com. https://study.com/academy/lesson/calculating-percent-composition-and-determining-empirical-formulas.html

Percent Composition Calculator. (n.d.). https://www.chemhaven.org/che101/tools/percentcomp/percentcomp.cgi

Percentage composition: formula, determination, examples, videos. (2019, November 21). Toppr-guides. https://www.toppr.com/guides/chemistry/some-basic-concepts-of-chemistry/percentage-composition/

Periodic Table - Ptable. (n.d.). Properties. https://ptable.com/?lang=en#Properties

PubChem. (n.d.). Periodic Table of elements. PubChem. https://pubchem.ncbi.nlm.nih.gov/periodic-table/

Science, C. (2024, November 2). Percent composition. CK-12 Foundation. https://flexbooks.ck12.org/cbook/ck-12-chemistry-flexbook-2.0/section/10.10/primary/lesson/percent-composition-chem/

Silberberg, M. S., Amateis, P. G. (2021). Chemistry: The molecular nature of matter and change (9th ed.). McGraw-Hill Education

Study.com (2024) Chemistry 101: General Chemistry| Anton Lavoisier| Importance, Experiments and Atomic Theory https://study.com/academy/lesson/antoine-lavoisier-atomic-theory-contribution.html?srsltid

The Editors of Encyclopaedia Britannica. (2024, October 21). Avogadro’s law | Definition, Explanation, & Facts. Encyclopedia Britannica. https://www.britannica.com/science/Avogadros-law


 DOWNLOADABLE MODULES

TOPIC: MASS


TOPIC: MOLE

 


TOPIC: PERCENT COMPOSITION

KimikApp Mole Concept Post-test

KimikApp Mole Concept Post-Test

1. How many particles are in one mole of any substance?

  • a. 6.02 x 10²³
  • b. 1.00 x 10²³
  • c. 3.01 x 10²³
  • d. 9.02 x 10²³
Correct Answer: a - This is Avogadro's number, representing the number of particles in one mole.

2. What is the SI unit used to express the amount of a substance?

  • a. Liter
  • b. Mole
  • c. Gram
  • d. Joule
Correct Answer: b - Mole is the SI unit for amount of substance, defining a set number of particles.

3. Which is the molar mass of \(H_2O\)?

  • a. 18 g/mol
  • b. 10 g/mol
  • c. 20 g/mol
  • d. 22 g/mol
Correct Answer: a - The molar mass of water is calculated as 2 hydrogen atoms (1 g/mol each) + 1 oxygen atom (16 g/mol) = 18 g/mol.

4. If you have 2 moles of water (H₂O) how many molecules of water do you have?

  • a. 1.20 x 10²³
  • b. 1.20 x 10²⁴
  • c. 2.41 x 10²³
  • d. 3.21 x 10²⁴
Correct Answer: b - Since one mole contains 6.02 x 10²³ molecules, two moles have twice that amount, or 1.20 x 10²⁴ molecules.

5. What is Avogadro's number?

  • a. 1.00 x 10²³
  • b. 6.02 x 10²²
  • c. 6.02 x 10²³
  • d. 3.01 x 10²⁴
Correct Answer: c - Avogadro's number is defined as 6.02 x 10²³, the number of particles in one mole of a substance.

6. If you have 1 mole of carbon atoms, how much mass does it represent if the atomic mass of carbon is 12 g/mol?

  • a. 12 g
  • b. 24 g
  • c. 6 g
  • d. 18 g
Correct Answer: a - One mole of carbon atoms has a mass of 12 g, which is the atomic mass of carbon.

7. What does it mean when we say that a substance has 1 mole of particles?

  • a. The substance contains 6.02 x 10²³ particles.
  • b. The substance weighs exactly 1 gram.
  • c. The substance has the same mass as any other mole of substances.
  • d. The substance reacts with 1 liter of another substance.
Correct Answer: a - One mole of any substance contains exactly 6.02 x 10²³ particles, regardless of the substance.

8. If the molar mass of carbon dioxide (CO₂) is 44 g/mol, how much mass does 2 moles of CO₂ have?

  • a. 22 g
  • b. 44 g
  • c. 88 g
  • d. 132 g
Correct Answer: c - Since 1 mole of CO₂ has a mass of 44 g, 2 moles would have a mass of 88 g (2 x 44 g).

9. A sample contains 4.0 moles of carbon. How many grams of carbon are present if the molar mass is 12 g/mol?

  • a. 24 g
  • b. 36 g
  • c. 48 g
  • d. 12 g
Correct Answer: c - 4 moles of carbon would have a mass of 48 g (4 x 12 g).

10. How many moles of hydrogen are present in 2 grams of H₂? (Molar mass of H₂ is 2 g/mol.)

  • a. 1 mole
  • b. 2 moles
  • c. 0.5 moles
  • d. 4 moles
Correct Answer: a - Since 1 mole of H₂ weighs 2 g, 2 g of H₂ is equal to 1 mole.

11. What is the molar mass of NaCl if Na has a molar mass of 23 g/mol and Cl has 35.5 g/mol?

  • a. 58.5 g/mol
  • b. 45 g/mol
  • c. 59 g/mol
  • d. 57 g/mol
Correct Answer: a - The molar mass of NaCl is the sum of Na (23 g/mol) and Cl (35.5 g/mol), which is 58.5 g/mol.

12. How many grams are there in 3 moles of water H₂O? (Molar mass = 18 g/mol)

  • a. 18 g
  • b. 36 g
  • c. 54 g
  • d. 72 g
Correct Answer: c - 3 moles of H₂O is 3 x 18 g, which equals 54 g.

13. If you have a sample of 3.0 moles of nitrogen gas (N₂), what is the mass of this sample? (Molar mass of nitrogen is 28 g/mol.)

  • a. 28 g
  • b. 56 g
  • c. 84 g
  • d. 112 g
Correct Answer: c - The mass of 3 moles of N₂ is 3 x 28 g, which is 84 g.

14. A chemist needs 0.5 moles of sulfuric acid (H₂SO₄). The molar mass of H₂SO₄ is 98 g/mol. How many grams of sulfuric acid does the chemist need?

  • a. 49 g
  • b. 98 g
  • c. 196 g
  • d. 25 g
Correct Answer: a - 0.5 moles of H₂SO₄ has a mass of 0.5 x 98 g, which equals 49 g.

15. If 3.01 x 10²³ molecules of glucose (C₆H₁₂O₆) weigh 90 grams, how much would one mole of glucose weigh?

  • a. 45 grams
  • b. 90 grams
  • c. 180 grams
  • d. 360 grams
Correct Answer: c - Since 3.01 x 10²³ molecules is half of Avogadro's number, doubling 90 grams gives us 180 grams per mole.

16. Which of the following describes percentage composition?

  • a. The ratio of the mass of each element to the mass of the compound.
  • b. The total number of atoms in a molecule.
  • c. The percentage of atoms in the periodic table.
  • d. The percentage of chemical bonds in a compound.
Correct Answer: a - Percentage composition represents the mass ratio of each element in a compound.

17. How do you calculate the percentage composition of a compound?

  • a. Divide the molar mass by the number of atoms.
  • b. Divide the mass of each element by the molar mass of the compound and multiply by 100.
  • c. Divide the number of molecules by the number of moles.
  • d. Divide the mass of the sample by Avogadro's number.
Correct Answer: b - Percentage composition is found by dividing the mass of each element by the compound’s molar mass, then multiplying by 100.

18. What is the molar mass of NaCl?

  • a. 22.99 g/mol
  • b. 35.45 g/mol
  • c. 58.44 g/mol
  • d. 23.99 g/mol
Correct Answer: c - The molar mass of NaCl is the sum of Na (22.99 g/mol) and Cl (35.45 g/mol), which is approximately 58.44 g/mol.

19. In a water molecule (H₂O), what is the mass percentage of hydrogen?

  • a. 11.19%
  • b. 88.81%
  • c. 20.00%
  • d. 33.33%
Correct Answer: a - In water, hydrogen’s mass percentage is about 11.19%, with oxygen making up the remaining 88.81%.

20. What is the percentage of nitrogen in NH₃ (Molar mass of NH₃ is 17 g/mol, nitrogen is 14 g/mol)?

  • a. 14%
  • b. 18%
  • c. 82%
  • d. 70%
Correct Answer: c - Nitrogen makes up approximately 82% of NH₃'s molar mass (14/17 x 100).

21. What is the molar mass of CO₂?

  • a. 12 g/mol
  • b. 16 g/mol
  • c. 32 g/mol
  • d. 44 g/mol
Correct Answer: d - The molar mass of CO₂ is the sum of C (12 g/mol) and two O atoms (2 x 16 g/mol), which is 44 g/mol.

22. How many moles of H₂O are in 36 grams of water? (Molar mass of H₂O is 18 g/mol)

  • a. 1 mole
  • b. 2 moles
  • c. 3 moles
  • d. 4 moles
Correct Answer: b - 36 grams of water is 36/18 = 2 moles.

23. Which compound has the highest percentage of oxygen?

  • a. CO₂
  • b. H₂O
  • c. H₂O₂
  • d. O₂
Correct Answer: d - O₂ has the highest oxygen percentage by mass, with oxygen constituting about 100% of its molar mass.

24. What is the empirical formula for C₆H₁₂O₆?

  • a. CH₂O
  • b. CHO
  • c. C₆HO
  • d. C₆H₁₂O₆
Correct Answer: a - The empirical formula of C₆H₁₂O₆ is CH₂O, as it represents the simplest whole-number ratio of elements.

25. How many molecules are there in 2 moles of H₂?

  • a. 3.01 x 10²³
  • b. 6.02 x 10²³
  • c. 1.20 x 10²⁴
  • d. 2.4 x 10²⁴
Correct Answer: c - 2 moles contain 2 x 6.02 x 10²³ molecules, which equals 1.20 x 10²⁴ molecules.

26. Which element has a molar mass of approximately 1 g/mol?

  • a. Helium
  • b. Hydrogen
  • c. Carbon
  • d. Oxygen
Correct Answer: b - Hydrogen has a molar mass of approximately 1 g/mol.

27. Which quantity represents Avogadro's number?

  • a. 6.022 x 10²³ atoms/mole
  • b. 6.022 x 10²² atoms/mole
  • c. 6.022 x 10²⁴ atoms/mole
  • d. 6.022 x 10²¹ atoms/mole
Correct Answer: a - Avogadro's number is 6.022 x 10²³ atoms or molecules per mole.

28. What is the mass of 1 mole of NH₃?

  • a. 17 g
  • b. 18 g
  • c. 19 g
  • d. 20 g
Correct Answer: a - The molar mass of NH₃ is 14 (N) + (3 x 1) = 17 g/mol.

29. If 1 mole of CO₂ has a mass of 44 grams, what is the mass of 0.5 moles of CO₂?

  • a. 11 g
  • b. 22 g
  • c. 33 g
  • d. 44 g
Correct Answer: b - Half a mole of CO₂ would weigh half of 44 grams, which is 22 grams.

30. The atomic mass of chlorine (Cl) is approximately 35.5. How many grams are in 2 moles of Cl?

  • a. 17.75 g
  • b. 35.5 g
  • c. 71 g
  • d. 142 g
Correct Answer: c - Since the atomic mass of Cl is 35.5 grams per mole, multiplying it by 2 moles gives 71 grams.

Your score is:

GENERAL OVERVIEW

In our everyday life, we often find that measuring or quantifying items is essential, whether it’s for purchasing goods, cooking, or managing resources. The method of quantification depends on what’s more practical in the given situation. For example, when buying produce at the market, vendors typically sell grains, like rice or mung beans, by weight, using a scale to measure their mass. On the other hand, they sell items like eggs by counting the number of individual pieces. The choice between measuring by mass or by counting largely depends on convenience and practicality. It's far easier to measure the mass of a large quantity of small items, such as rice grains, than to count each one individually. In contrast, when dealing with relatively larger, distinguishable items like eggs, it’s more straightforward to count them rather than measure their weight. To represent these quantities, we use mass units such as grams or kilograms for weight, and counting units like a dozen, case, or package for discrete items.

In scientific contexts, particularly in chemistry, measuring substances becomes a more precise and specialized process. Chemists often need to measure specific quantities of materials to conduct reactions and produce new compounds. Unlike market goods, the substances involved in chemical reactions are made up of atoms, ions, or molecules—particles that are far too small to be counted directly. To overcome this challenge, chemists use a unit called the mole to represent a specific number of these tiny particles. The mole allows chemists to "count" these particles by mass, which is far more practical. Much like how we use a dozen to represent 12 items, a mole represents a specific number of particles—6.022 × 10²³ particles, a quantity known as Avogadro’s number. This unit is essential in bridging the microscopic world of atoms and molecules with the macroscopic world we can measure.

Without the mole, chemical reactions would be extremely difficult to measure because the quantities of atoms or molecules involved are so vast that counting them would be impossible. Instead, by using the mole concept, chemists can weigh out a substance and know exactly how many atoms, ions, or molecules are present. The mole helps to simplify complex chemical calculations, enabling precise formulation of compounds and the prediction of reaction outcomes. It’s also the key to understanding concepts such as molar mass, the mass of one mole of a substance, which allows chemists to relate the mass of a substance to the number of particles it contains.

Learning Competencies/Objectives: 

  • use the mole concept to express mass of substances; and
  • determine the percentage composition of a compound given its chemical formula and vice-versa. 

To start, we encourage you to take the pre-assessment provided. It will help you identify what you already know and where you might need further study before proceeding with the Application's lessons. Through this journey, you will gain a deeper understanding of how the mole connects the world of the very small to the world of the observable, and how it’s used to solve problems in chemistry.


KimikApp Mole Concept Pre-test

KimikApp Mole Concept Pre-Assessment

1. How many particles are in one mole of any substance?

  • a. 6.02 x 10²³
  • b. 1.00 x 10²³
  • c. 3.01 x 10²³
  • d. 9.02 x 10²³
Correct Answer: a - This is Avogadro's number, representing the number of particles in one mole.

2. What is the SI unit used to express the amount of a substance?

  • a. Liter
  • b. Mole
  • c. Gram
  • d. Joule
Correct Answer: b - Mole is the SI unit for amount of substance, defining a set number of particles.

3. Which is the molar mass of \(H_2O\)?

  • a. 18 g/mol
  • b. 10 g/mol
  • c. 20 g/mol
  • d. 22 g/mol
Correct Answer: a - The molar mass of water is calculated as 2 hydrogen atoms (1 g/mol each) + 1 oxygen atom (16 g/mol) = 18 g/mol.

4. If you have 2 moles of water (H₂O) how many molecules of water do you have?

  • a. 1.20 x 10²³
  • b. 1.20 x 10²⁴
  • c. 2.41 x 10²³
  • d. 3.21 x 10²⁴
Correct Answer: b - Since one mole contains 6.02 x 10²³ molecules, two moles have twice that amount, or 1.20 x 10²⁴ molecules.

5. What is Avogadro's number?

  • a. 1.00 x 10²³
  • b. 6.02 x 10²²
  • c. 6.02 x 10²³
  • d. 3.01 x 10²⁴
Correct Answer: c - Avogadro's number is defined as 6.02 x 10²³, the number of particles in one mole of a substance.

6. If you have 1 mole of carbon atoms, how much mass does it represent if the atomic mass of carbon is 12 g/mol?

  • a. 12 g
  • b. 24 g
  • c. 6 g
  • d. 18 g
Correct Answer: a - One mole of carbon atoms has a mass of 12 g, which is the atomic mass of carbon.

7. What does it mean when we say that a substance has 1 mole of particles?

  • a. The substance contains 6.02 x 10²³ particles.
  • b. The substance weighs exactly 1 gram.
  • c. The substance has the same mass as any other mole of substances.
  • d. The substance reacts with 1 liter of another substance.
Correct Answer: a - One mole of any substance contains exactly 6.02 x 10²³ particles, regardless of the substance.

8. If the molar mass of carbon dioxide (CO₂) is 44 g/mol, how much mass does 2 moles of CO₂ have?

  • a. 22 g
  • b. 44 g
  • c. 88 g
  • d. 132 g
Correct Answer: c - Since 1 mole of CO₂ has a mass of 44 g, 2 moles would have a mass of 88 g (2 x 44 g).

9. A sample contains 4.0 moles of carbon. How many grams of carbon are present if the molar mass is 12 g/mol?

  • a. 24 g
  • b. 36 g
  • c. 48 g
  • d. 12 g
Correct Answer: c - 4 moles of carbon would have a mass of 48 g (4 x 12 g).

10. How many moles of hydrogen are present in 2 grams of H₂? (Molar mass of H₂ is 2 g/mol.)

  • a. 1 mole
  • b. 2 moles
  • c. 0.5 moles
  • d. 4 moles
Correct Answer: a - Since 1 mole of H₂ weighs 2 g, 2 g of H₂ is equal to 1 mole.

11. What is the molar mass of NaCl if Na has a molar mass of 23 g/mol and Cl has 35.5 g/mol?

  • a. 58.5 g/mol
  • b. 45 g/mol
  • c. 59 g/mol
  • d. 57 g/mol
Correct Answer: a - The molar mass of NaCl is the sum of Na (23 g/mol) and Cl (35.5 g/mol), which is 58.5 g/mol.

12. How many grams are there in 3 moles of water H₂O? (Molar mass = 18 g/mol)

  • a. 18 g
  • b. 36 g
  • c. 54 g
  • d. 72 g
Correct Answer: c - 3 moles of H₂O is 3 x 18 g, which equals 54 g.

13. If you have a sample of 3.0 moles of nitrogen gas (N₂), what is the mass of this sample? (Molar mass of nitrogen is 28 g/mol.)

  • a. 28 g
  • b. 56 g
  • c. 84 g
  • d. 112 g
Correct Answer: c - The mass of 3 moles of N₂ is 3 x 28 g, which is 84 g.

14. A chemist needs 0.5 moles of sulfuric acid (H₂SO₄). The molar mass of H₂SO₄ is 98 g/mol. How many grams of sulfuric acid does the chemist need?

  • a. 49 g
  • b. 98 g
  • c. 196 g
  • d. 25 g
Correct Answer: a - 0.5 moles of H₂SO₄ has a mass of 0.5 x 98 g, which equals 49 g.

15. If 3.01 x 10²³ molecules of glucose (C₆H₁₂O₆) weigh 90 grams, how much would one mole of glucose weigh?

  • a. 45 grams
  • b. 90 grams
  • c. 180 grams
  • d. 360 grams
Correct Answer: c - Since 3.01 x 10²³ molecules is half of Avogadro's number, doubling 90 grams gives us 180 grams per mole.

16. Which of the following describes percentage composition?

  • a. The ratio of the mass of each element to the mass of the compound.
  • b. The total number of atoms in a molecule.
  • c. The percentage of atoms in the periodic table.
  • d. The percentage of chemical bonds in a compound.
Correct Answer: a - Percentage composition represents the mass ratio of each element in a compound.

17. How do you calculate the percentage composition of a compound?

  • a. Divide the molar mass by the number of atoms.
  • b. Divide the mass of each element by the molar mass of the compound and multiply by 100.
  • c. Divide the number of molecules by the number of moles.
  • d. Divide the mass of the sample by Avogadro's number.
Correct Answer: b - Percentage composition is found by dividing the mass of each element by the compound’s molar mass, then multiplying by 100.

18. What is the molar mass of NaCl?

  • a. 22.99 g/mol
  • b. 35.45 g/mol
  • c. 58.44 g/mol
  • d. 23.99 g/mol
Correct Answer: c - The molar mass of NaCl is the sum of Na (22.99 g/mol) and Cl (35.45 g/mol), which is approximately 58.44 g/mol.

19. In a water molecule (H₂O), what is the mass percentage of hydrogen?

  • a. 11.19%
  • b. 88.81%
  • c. 20.00%
  • d. 33.33%
Correct Answer: a - In water, hydrogen’s mass percentage is about 11.19%, with oxygen making up the remaining 88.81%.

20. What is the percentage of nitrogen in NH₃ (Molar mass of NH₃ is 17 g/mol, nitrogen is 14 g/mol)?

  • a. 14%
  • b. 18%
  • c. 82%
  • d. 70%
Correct Answer: c - Nitrogen makes up approximately 82% of NH₃'s molar mass (14/17 x 100).

21. What is the molar mass of CO₂?

  • a. 12 g/mol
  • b. 16 g/mol
  • c. 32 g/mol
  • d. 44 g/mol
Correct Answer: d - The molar mass of CO₂ is the sum of C (12 g/mol) and two O atoms (2 x 16 g/mol), which is 44 g/mol.

22. How many moles of H₂O are in 36 grams of water? (Molar mass of H₂O is 18 g/mol)

  • a. 1 mole
  • b. 2 moles
  • c. 3 moles
  • d. 4 moles
Correct Answer: b - 36 grams of water is 36/18 = 2 moles.

23. Which compound has the highest percentage of oxygen?

  • a. CO₂
  • b. H₂O
  • c. H₂O₂
  • d. O₂
Correct Answer: d - O₂ has the highest oxygen percentage by mass, with oxygen constituting about 100% of its molar mass.

24. What is the empirical formula for C₆H₁₂O₆?

  • a. CH₂O
  • b. CHO
  • c. C₆HO
  • d. C₆H₁₂O₆
Correct Answer: a - The empirical formula of C₆H₁₂O₆ is CH₂O, as it represents the simplest whole-number ratio of elements.

25. How many molecules are there in 2 moles of H₂?

  • a. 3.01 x 10²³
  • b. 6.02 x 10²³
  • c. 1.20 x 10²⁴
  • d. 2.4 x 10²⁴
Correct Answer: c - 2 moles contain 2 x 6.02 x 10²³ molecules, which equals 1.20 x 10²⁴ molecules.

26. Which element has a molar mass of approximately 1 g/mol?

  • a. Helium
  • b. Hydrogen
  • c. Carbon
  • d. Oxygen
Correct Answer: b - Hydrogen has a molar mass of approximately 1 g/mol.

27. Which quantity represents Avogadro's number?

  • a. 6.022 x 10²³ atoms/mole
  • b. 6.022 x 10²² atoms/mole
  • c. 6.022 x 10²⁴ atoms/mole
  • d. 6.022 x 10²¹ atoms/mole
Correct Answer: a - Avogadro's number is 6.022 x 10²³ atoms or molecules per mole.

28. What is the mass of 1 mole of NH₃?

  • a. 17 g
  • b. 18 g
  • c. 19 g
  • d. 20 g
Correct Answer: a - The molar mass of NH₃ is 14 (N) + (3 x 1) = 17 g/mol.

29. If 1 mole of CO₂ has a mass of 44 grams, what is the mass of 0.5 moles of CO₂?

  • a. 11 g
  • b. 22 g
  • c. 33 g
  • d. 44 g
Correct Answer: b - Half a mole of CO₂ would weigh half of 44 grams, which is 22 grams.

30. The atomic mass of chlorine (Cl) is approximately 35.5. How many grams are in 2 moles of Cl?

  • a. 17.75 g
  • b. 35.5 g
  • c. 71 g
  • d. 142 g
Correct Answer: c - Since the atomic mass of Cl is 35.5 grams per mole, multiplying it by 2 moles gives 71 grams.

Your score is:

KimikApp is an innovative web-based learning application developed by Bachelor of Secondary Education students at Camarines Norte State College. Created specifically to support Grade 9 Chemistry students, KimikApp supplements the curriculum by offering an interactive and engaging way to master essential Chemistry topics, particularly the Mole Concept. KimikApp addresses various learning preferences, allowing students to choose how they engage with the material through a range of resources tailored to visual, auditory, and kinesthetic learning styles.

Key Features:

  • Video Lessons: Concise instructional videos clarify complex topics, making Chemistry concepts accessible and understandable.
  • Podcasts: Engaging audio content allows students to review lessons or gain insights into Chemistry concepts on the go, providing an alternative to visual learning.
  • Interactive Quizzes: Formative assessments help students test their knowledge and track their progress, providing immediate feedback for continuous improvement.
  • Simulations and Visualizations: Realistic simulations enable students to actively engage with Chemistry principles, enhancing hands-on understanding.
  • Images and Visual Aids: High-quality images and infographics simplify and illustrate abstract concepts, aiding visual learners in retaining complex information
  • Activities: Practical activities encourage students to apply their knowledge, promoting critical thinking and hands-on learning experiences beyond the screen.

These features create a supportive, self-paced environment that encourages students to deepen their understanding and improve their performance in Chemistry. With KimikApp, we hope to spark curiosity and inspire confidence in Chemistry learners.


 User's Manual

Below are the User Manuals for Students and Teachers. These guides provide instructions for navigating and making the most out of KimikApp. The Student Manual outlines how to access lessons, quizzes, podcasts, and interactive activities, ensuring students can maximize their learning experience. The Teacher Manual offers guidance on utilizing the app’s features for instruction and answers to activities for checking, accessing the Teacher’s Guide, and using verification codes to unlock additional resources. Both manuals are crafted to help users engage with the app seamlessly and support their roles in the Chemistry learning process.


Student's Guide Access

This guide is for students. Click the button below to access the resources.

Teacher's Guide Access

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Welcome to KimikApp, a dedicated e-learning platform designed to enhance Grade 9 students' understanding of Chemistry. KimikApp focuses on tackling challenging topics, particularly the Mole Concept, by integrating technology and engaging students through interactive resources. This application was developed in response to challenges students encounter with complex Chemistry topics when traditional teaching materials prove insufficient. KimikApp is crafted to cater to diverse learning styles, making Chemistry more accessible, engaging, and enjoyable for students as they progress at their own pace.

With features like instructional videos, interactive quizzes, podcasts, and visual aids, KimikApp offers a comprehensive learning experience that transforms abstract Chemistry concepts into clear, graspable knowledge. We aim for this platform to be a valuable learning tool, supporting students in building a strong Chemistry foundation.

We hope you have a rewarding and enjoyable experience with the app!

    

 Lesson 1: Mass

I. Objectives

At the end of the lesson, students will be able to:

  1. Differentiate between Total Count and Mass
  2. Compute Molar Mass 
  3. Apply molar mass formula to solve real world problems.

II. Subject Matter

  • Topic: Mass
  • Materials: Digital balance simulator, visual aids, interactive mass unit converter
  • References: E-learning platform, textbook, online simulation tools


III. Learning Activities

Motivational Activity

 

Lesson Proper

A. Visual Learners

Overview

     The Mass in Mole Concept is a foundational idea in chemistry that links the microscopic world of atoms and molecules to measurable quantities in the laboratory. It allows chemists to quantify substances in terms of both mass and the number of particles, providing a way to work with atoms and molecules in practical amounts. The key to this concept is the mole, a unit that represents 6.022×10^23 particles, known as Avogadro’s number. By defining a standard relationship between mass and particle count, the mole concept enables chemists to precisely calculate how much of a substance is involved in a reaction. This relationship is further simplified by *molar mass*, the mass of one mole of any given substance, which allows for easy conversion between the grams of a substance and the moles it contains. Understanding the Mass in Mole Concept is crucial for analyzing chemical reactions, determining reactant and product amounts, and exploring how elements and compounds interact on both small and large scales.

Importance of Measuring Mass in Everyday Life and Scientific Applications

Cooking

    While not always explicitly acknowledged, the mole concept also plays a role in cooking, especially in baking, where the proportions of ingredients matter. Understanding the relationship between mass and quantity can ensure that ingredients combine in the right ratios, yielding desired textures and flavors. For example, balancing acids and bases in baking (like baking soda and vinegar) relies on the mole concept to avoid excess or deficiency, which could affect both taste and texture.

 Health and Fitness

    In health and fitness, understanding the mass in mole concept can help in calculating the body's metabolic processes. For instance, the breakdown of carbohydrates, proteins, and fats involves precise biochemical reactions, where knowing the molar quantities of nutrients and energy molecules (like ATP) is crucial. This aids in designing diets and understanding caloric intake based on the body's needs at the molecular level.

Chemistry


    In chemistry, the mass in mole concept is fundamental for nearly all chemical calculations. It allows chemists to balance reactions, calculate reactant and product masses, and analyze reaction yields. By converting between mass and moles, chemists can precisely predict how substances will interact, control reaction conditions, and ensure that chemical processes are efficient and environmentally friendly.

Physics

In physics, the mole concept aids in calculations involving gases and thermodynamics. The ideal gas law, for example, 
PV=nRTPV = nRT

 

Medicine

In medicine, accurate dosing is essential, and the mole concept plays a critical role in determining the correct amounts of drugs. Pharmacists and doctors use molar mass to convert prescribed doses into precise weights, ensuring that patients receive effective but safe amounts. This is especially vital for medications requiring exact dosages, such as chemotherapy drugs or insulin, where even slight variations could impact treatment efficacy or patient safety.

Differentiating Total Count and Mass


Computing Molar Mass 

Now, let’s delve into the computations! Learn the step-by-step process to calculate molar mass, followed by practical examples with compounds like H₂O, CO₂, and NaCl to solidify your understanding.



Power point Presentation  

VIDEO DISCUSSION:
        This video discussion delves into the concept of mass in moles, exploring its historical foundation, definition, and significance in chemistry. We’ll examine how this principle connects measurable quantities to atomic-scale particles, crucial for calculations in chemical reactions. Starting with key figures like Lavoisier, Dalton, Avogadro, and Cannizzaro, we trace the development of the mole and Avogadro's number. We’ll discuss calculating molar mass, differentiating between total particle count and mass, and applying these principles through practical examples and situational problems. Join us as we bridge the atomic world with our everyday reality.


b. Auditory

        Hello there! I’m Chain D. Habana, and welcome to KimiKapp Podcast! Today, we’re diving into the mass-in-mole concept—a key chemistry idea that links measurable amounts to the atomic world. We’ll explore its historical roots from Lavoisier’s mass conservation to Avogadro's number, defining the mole as a unit for counting particles. This concept is vital for precise measurements in chemical reactions. We’ll also cover how to calculate molar mass with examples, like finding 17 grams per mole for NH₃. Thanks for tuning in, and keep exploring with KimiKapp Podcast!

c. Kinesthetic
        Kindly do the  learning activities and follow the instructions.

Click here to access the link for the worksheets.

Instructions:

  1. Locate the link to the online worksheet provided below the image presented.
  2. Open the worksheet and carefully review the tasks.
  3. Complete Activity 1, 2, and 4 from the worksheet.
  4. Write your answers on one whole sheet of paper.
  5. Ensure your answers are neat and clear before submission. Good luck!

Additional Activity! 

Think-Pair-Share Activity:"Weighing and Converting Mass"

Click here to access the link for the Reading Scale Simulator

Objective:

    In pairs, you will use a virtual balance to weigh different objects and then convert your findings into different mass units using an online converter tool.

Materials Needed:

  • Access to a computer or tablet with internet access
  • Virtual balance website (Reading Scale Simulator)
  • Online mass converter tool.
  • Paper and pen for recording measurements

Instructions:

1. The students will find a partner to work with for this Think-Pair-Share Activity.

2. After the students have their own respective pair, the students will now access the provided link at the bottom part of the image. 

3. Once the pair of students have accessed the link, they will now choose different objects from the list provided (e.g., $1 coin, apple and pineapple) to weigh using the virtual balance.

4. Use the virtual balance to weigh each object. Record the mass in kilograms (kg) on your one whole sheet of paper.

5. After measuring the mass of each object, navigate the provided mass converter tool. Input the mass you recorded and select the desired unit to convert ( kilograms to grams) Write down the converted values.

6.  Share your recorded measurements and converted values with your partner.  Discuss any differences you observed and the importance of converting between mass units.

Generalization/Summary 

    The concept of mass in mole connects the measurable mass of a substance to the number of particles it contains, which is essential in chemistry. Mass refers to the amount of matter in a substance, and it’s usually measured in grams (g). The mole, on the other hand, is a counting unit that represents 6.022 x 10²³ particles (Avogadro's number), whether they are atoms, molecules, or ions. By knowing the molar mass of a substance, we can convert between the mass of a sample and the number of particles it contains. For example, 18 grams of water (H₂O) is equivalent to one mole, containing approximately 6.022 x 10²³ water molecules.

    Understanding the molar mass of compounds enables chemists to perform accurate calculations for chemical reactions, balancing equations, and preparing precise quantities for experiments. Whether it’s in pharmaceuticals, materials science, or daily life applications, the mass-in-mole concept is central to converting between the macroscopic (grams) and microscopic (particles) worlds.


Assignment/Task     

Formative Assessment: