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Chapter 5 Part 6 : Test

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Lesson 30


Chapter 5 Part 6


🎉🎉🎉 PARTY PEOPLE! Welcome to the grand finale of our Gaseous Journey 🚀... the QUIZ TIME!! Remember, all you need is to achieve 70% to pass this exam. So, buckle up and let's do this! 🎉🎉🎉

⭐⭐⭐ Multiple Choice Questions ⭐⭐⭐ Please choose the most suitable answer for each question.

  1. What does the term "effusion" refer to in the context of gases? 🌬️ A. Mixing of gases B. Passage of a gas through a tiny orifice C. The spread of a gas throughout space D. The dissolving of gas in a liquid

  2. If two gases are at the same temperature, how do their average kinetic energies compare? ⚖️ A. They're the same. B. The lighter gas has a higher kinetic energy. C. The heavier gas has a higher kinetic energy. D. Cannot be determined without more information.

  3. According to Charles’ Law, if the volume of a gas decreases, what happens to the temperature, provided pressure remains constant? 🌡️ A. The temperature decreases. B. The temperature increases. C. The temperature remains the same. D. Cannot be determined without more information.

  4. In an ideal gas, what relationship does Boyle's law describe? ⛽ A. The pressure is directly proportional to the volume at constant temperature. B. The pressure is inversely proportional to the volume at constant temperature. C. The pressure is directly proportional to the temperature at constant volume. D. The pressure is inversely proportional to the temperature at constant volume.

  5. What is the ratio of number of moles of a specific gas to the total number of moles known as? 👩‍🔬 A. Mole fraction B. Molar volume C. Molar mass D. Molar ratio

  6. At the same temperature, a lighter gas particle moves… 🎈 A. Slower than a heavier one B. Faster than a heavier one C. At the same speed as a heavier one D. Cannot be determined without more information

  7. If we double the absolute temperature of a fixed volume of a gas, what happens to the pressure? 🎛️ A. It doubles. B. It halves. C. It remains the same. D. It quadruples.

  8. What does the universal gas constant (R) stand for in the ideal gas law equation PV = nRT? 🌍 A. Ratio of pressure and volume B. Rate of gas effusion C. Reactivity of the gas D. Proportionality constant

  9. What happens when real gases are under high pressure and low temperature?❄️ A. They deviate more from ideal behavior. B. They behave exactly like ideal gases. C. Their particles move faster. D. Their particles exert no forces on each other.

  10. What is the process of the spread of a gas throughout space called? 🌌 A. Compression B. Expansion C. Diffusion D. Condensation

Remember, no peaking at the answers! Only check them after you're done!

📝📝📝 Fill in the Blanks 📝📝📝

  1. The sum of mole fractions of a gas mixture is always _________.

  2. The _____ _____ is a hypothetical gas that follows the gas laws at all temperatures and pressures.

  3. The direct relationship between the absolute temperature and volume of a gas at constant pressure is known as _________’s Law.

  4. The average kinetic energy of gas particles is directly proportional to _________.

  5. According to the _________ Law, the rate of effusion of a gas is inversely proportional to the square root of its molar mass.

  6. The unit of pressure in the International System of Units (SI) is _________.

  7. In the kinetic theory of gases, the gas pressure results from gas molecules _________ the walls of the container.

  8. When comparing the speed of two gases at the same temperature, the ratio can be calculated as √(M2/M1), where M1 and M2 are the molar masses of the gases. This concept is known as _________.

  9. According to the ideal gas law, if the number of moles and temperature of a gas remain constant, its volume is _________ to its pressure.

  10. The combined gas law formula, P1V1/T1 = P2V2/T2, allows us to calculate changes in pressure, volume, and temperature, assuming the _________ of gas stays constant.

🤓🤓🤓 Problem Solving 🤓🤓🤓

  1. If a 2.0 L sample of oxygen at 0°C is heated at constant pressure until the volume is 2.5 L, what is the final temperature?

  2. A helium balloon has a volume of 20.0 L at sea level (1.0 atm). If it is released and rises to an altitude where the pressure is 0.60 atm, what will its new volume be, assuming constant temperature?

  3. Calculate the mole fraction of oxygen in a mixture that contains 28 g of nitrogen and 32 g of oxygen.

  4. Using the ideal gas law, calculate the number of moles in 22.4 liters of a gas at standard temperature and pressure (STP).

  5. Using Graham's law of effusion, if gas A (molar mass 4 g/mol) effuses twice as fast as gas B, what is the molar mass of gas B?

  6. If the temperature of a fixed quantity of gas is raised from 300K to 600K, what happens to the pressure, if the volume is kept constant?

  7. A sample of nitrogen is collected over water at 18.5°C. The vapor pressure of water at 18.5°C is 16 mm Hg. The water levels inside and outside the tube were equalized. If the atmospheric pressure is 756 mm Hg, what is the partial pressure of nitrogen?

  8. The rate of diffusion of a particular gas was measured and found to be 24 cm^3/min. Under the same conditions, the rate of diffusion of methane gas (CH4) was found to be 47.8 cm^3/min. What is the molar mass of the unknown gas?

  9. A sample of nitrogen gas was collected over water at 20°C and a total pressure of 1.00 atm. A total volume of 250 cm^3 was collected. What mass of nitrogen was collected? (At 20°C the vapor pressure of water is 17.5 mmHg).

  10. Calculate the molar mass of a gas if it took 5.0 s for 10 cm^3 of helium gas to effuse under certain conditions of temperature and pressure, and under the same conditions, it took the gas 20.0 s to effuse from the same orifice.

And that's the end! You've made it through! Now take a deep breath (remember, it's a mixture of gases 😉), check your answers, and keep the 70% rule in mind. You got this! 💪

Let me know when you're ready for the answers! 📝🤓🌈





Answers


Alright! Let's see how you did! 🧐💡

🤓🤓🤓 Multiple Choice Questions 🤓🤓🤓

  1. a) Decrease

  2. c) An increase in the pressure of the gas

  3. b) 273 K

  4. a) 1 atm

  5. b) 0.0821 L atm/mol K

  6. b) False

  7. c) The volume and pressure

  8. d) Kinetic Molecular Theory

  9. a) Effusion

  10. b) Helium

🧐🧐🧐 Fill in the Blanks 🧐🧐🧐 11. directly proportional

  1. ideal gas

  2. Charles

  3. temperature

  4. Graham's

  5. Pascal

  6. striking/colliding with

  7. Graham's Law

  8. inversely proportional

  9. quantity/amount

🤓🤓🤓 Problem Solving 🤓🤓🤓 21. 310 K

  1. 33.3 L

  2. 0.53

  3. 1 mole

  4. 16 g/mol

  5. The pressure would double.

  6. 740 mm Hg

  7. ~32 g/mol

  8. ~0.0103 g

  9. ~16 g/mol

Remember, the 70% rule: If you got at least 70% of the questions right (that's 21 out of 30), you are doing great! If not, don't worry, you've got what it takes to master this. Revisit the areas you struggled with and try again! 💪🌈🚀

Keep on being awesome, and remember, when it comes to learning, the sky's the limit! 🌠🌈🎉

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