Laurie LeBlanc Cuyamaca College Clicker Questions Chapter 11 Gases Laurie LeBlanc Cuyamaca College

A. The volume occupied by a gas is mostly empty space. All of the following are postulates of the kinetic molecular theory of gases EXCEPT: A. The volume occupied by a gas is mostly empty space. B. The average kinetic energy of the gas particles is proportional to the temperature in Celsius. C. The attraction/repulsion between gas molecules is very weak or negligible. D. Gas molecules or atoms move in a straight line between collisions. E. All of the above are correct postulates. Answer: B

A. The volume occupied by a gas is mostly empty space. All of the following are postulates of the kinetic molecular theory of gases EXCEPT: A. The volume occupied by a gas is mostly empty space. B. The average kinetic energy of the gas particles is proportional to the temperature in Celsius. C. The attraction/repulsion between gas molecules is very weak or negligible. D. Gas molecules or atoms move in a straight line between collisions. E. All of the above are correct postulates. Answer: B

Convert 580 mm Hg to units of atmospheres. A. 0.76 atm B. 1.00 atm C. 5.80 atm D. 0.763 atm E. 4.41 × 105 atm Answer: A

Convert 580 mm Hg to units of atmospheres. A. 0.76 atm B. 1.00 atm C. 5.80 atm D. 0.763 atm E. 4.41 × 105 atm Answer: A

Convert 35.5 psi to kPa. (Note: 1 atm = 14.7 psi; 1 atm = 101,325 Pa) A. 2.41 kPa B. 2.45 × 102 kPa C. 5.29 × 102 kPa D. 2.45 × 105 kPa E. 5.29 × 105 kPa Answer: B

Convert 35.5 psi to kPa. (Note: 1 atm = 14.7 psi; 1 atm = 101,325 Pa) A. 2.41 kPa B. 2.45 × 102 kPa C. 5.29 × 102 kPa D. 2.45 × 105 kPa E. 5.29 × 105 kPa Answer: B

A gas has a volume of 1. 0 L at 1 atm A gas has a volume of 1.0 L at 1 atm. By what factor must the pressure change in order to reduce the volume by half? (Assume the temperature is constant.) A. × 1 B. × 2 C. × 4 D. × 1/2 E. × 1/4 Answer: B

A gas has a volume of 1. 0 L at 1 atm A gas has a volume of 1.0 L at 1 atm. By what factor must the pressure change in order to reduce the volume by half? (Assume the temperature is constant.) A. × 1 B. × 2 C. × 4 D. × 1/2 E. × 1/4 Answer: B

A flask with 500. 0 mL of a gas is sealed on top of Mt A flask with 500.0 mL of a gas is sealed on top of Mt. Everest where the atmospheric pressure is 230. torr. What is the volume of the gas when the bottle is moved to sea level at a constant temperature? A. 651 mL B. 1.65 × 103 mL C. 0.151 mL D. 151 mL E. 500. mL Answer: D

A flask with 500. 0 mL of a gas is sealed on top of Mt A flask with 500.0 mL of a gas is sealed on top of Mt. Everest where the atmospheric pressure is 230. torr. What is the volume of the gas when the bottle is moved to sea level at a constant temperature? A. 651 mL B. 1.65 × 103 mL C. 0.151 mL D. 151 mL E. 500. mL Answer: D

B. The freezing point of hydrogen What is absolute zero? A. –273 °F B. The freezing point of hydrogen C. The x-intercept of a straight-line graph of V versus 1/P D. The x-intercept of a straight-line graph of V versus T E. The temperature of deep outer space Answer: D

B. The freezing point of hydrogen What is absolute zero? A. –273 °F B. The freezing point of hydrogen C. The x-intercept of a straight-line graph of V versus 1/P D. The x-intercept of a straight-line graph of V versus T E. The temperature of deep outer space Answer: D

A flexible container contains 1. 50 L of gas at 25 °C A flexible container contains 1.50 L of gas at 25 °C. What is the new volume when the container is heated to 100 °C at a constant pressure? A. 0.375 L B. 0.959 L C. 1.20 L D. 0.833 L E. 1.88 L Answer: E

A flexible container contains 1. 50 L of gas at 25 °C A flexible container contains 1.50 L of gas at 25 °C. What is the new volume when the container is heated to 100 °C at a constant pressure? A. 0.375 L B. 0.959 L C. 1.20 L D. 0.833 L E. 1.88 L Answer: E

A 36. 1 mL sample of oxygen gas contains 0. 529 mol of oxygen A 36.1 mL sample of oxygen gas contains 0.529 mol of oxygen. If enough oxygen is added to the sample to obtain a volume of 50.5 mL, what must the final mass of the sample be? (The pressure and temperature is constant.) A. 0.740 g B. 11.8 g C. 0.740 mol D. 23.7 g E. None of the above Answer: D

A 36. 1 mL sample of oxygen gas contains 0. 529 mol of oxygen A 36.1 mL sample of oxygen gas contains 0.529 mol of oxygen. If enough oxygen is added to the sample to obtain a volume of 50.5 mL, what must the final mass of the sample be? (The pressure and temperature is constant.) A. 0.740 g B. 11.8 g C. 0.740 mol D. 23.7 g E. None of the above Answer: D

What law is derived from the combined gas law under constant temperature and moles? A. Avogadro’s B. Charles’s C. Dalton’s D. Gay-Lussac’s E. Boyle’s Answer: E

What law is derived from the combined gas law under constant temperature and moles? A. Avogadro’s B. Charles’s C. Dalton’s D. Gay-Lussac’s E. Boyle’s Answer: E

A container with 1. 00 mol of gas is expanded from 5. 00 L to 10 A container with 1.00 mol of gas is expanded from 5.00 L to 10.0 L by adding more gas. How many moles of gas are present? (The temperature and pressure are kept constant.) A. 1.00 mol B. 2.00 mol C. 3.00 mol D. 5.00 mol E. 10.0 mol Answer: B

A container with 1. 00 mol of gas is expanded from 5. 00 L to 10 A container with 1.00 mol of gas is expanded from 5.00 L to 10.0 L by adding more gas. How many moles of gas are present? (The temperature and pressure are kept constant.) A. 1.00 mol B. 2.00 mol C. 3.00 mol D. 5.00 mol E. 10.0 mol Answer: B

A set of car tires contains a volume of 45. 5 L of air at 35 A set of car tires contains a volume of 45.5 L of air at 35.0 psi and 0.0 °C. When the car is driven, the temperature of the tires increases to 40.0 °C. What is the pressure (in psi) of each tire, assuming constant volume? A. 37.8 psi B. 35.0 psi C. 0 psi D. 40.1 psi E. 29.9 psi Answer: D

A set of car tires contains a volume of 45. 5 L of air at 35 A set of car tires contains a volume of 45.5 L of air at 35.0 psi and 0.0 °C. When the car is driven, the temperature of the tires increases to 40.0 °C. What is the pressure (in psi) of each tire, assuming constant volume? A. 37.8 psi B. 35.0 psi C. 0 psi D. 40.1 psi E. 29.9 psi Answer: D

How many moles of an ideal gas are in a container with a volume of 5 How many moles of an ideal gas are in a container with a volume of 5.5 L at 580 mm Hg and 20. °C? A. 1.3 mol B. 0.229 mol C. 0.174 mol D. 2.58 mol E. 0.17 mol Answer: E

How many moles of an ideal gas are in a container with a volume of 5 How many moles of an ideal gas are in a container with a volume of 5.5 L at 580 mm Hg and 20. °C? A. 1.3 mol B. 0.229 mol C. 0.174 mol D. 2.58 mol E. 0.17 mol Answer: E

What is the volume occupied by 28. 0 g of nitrogen gas at 1 What is the volume occupied by 28.0 g of nitrogen gas at 1.00 atm and 0.0 °C? A. 0.0295 L B. 1.00 L C. 22.4 L D. 48.8 L E. 0.0446 L Answer: C

What is the volume occupied by 28. 0 g of nitrogen gas at 1 What is the volume occupied by 28.0 g of nitrogen gas at 1.00 atm and 0.0 °C? A. 0.0295 L B. 1.00 L C. 22.4 L D. 48.8 L E. 0.0446 L Answer: C

A 4.17 g sample of a diatomic gas at 38 °C has a volume of 1.5 L at 1.00 atm. Identify the gas. A. H2 B. N2 C. F2 D. O2 E. Cl2 Answer: E

A 4.17 g sample of a diatomic gas at 38 °C has a volume of 1.5 L at 1.00 atm. Identify the gas. A. H2 B. N2 C. F2 D. O2 E. Cl2 Answer: E

A real gas can approach ideal behavior A. when both the pressure and temperature are high. B. when the pressure is high and the temperature is low. C. when both the pressure and temperature are low. D. when the pressure is low and the temperature is high. E. Real gases have ideal behavior no matter what the conditions are. Answer: D

A real gas can approach ideal behavior A. when both the pressure and temperature are high. B. when the pressure is high and the temperature is low. C. when both the pressure and temperature are low. D. when the pressure is low and the temperature is high. E. Real gases have ideal behavior no matter what the conditions are. Answer: D

Calculate the molar mass of a gas that has a density of 1 Calculate the molar mass of a gas that has a density of 1.70 g/L at STP. A. 2.02 g/mol B. 4.00 g/mol C. 28.0 g/mol D. 32.0 g/mol E. 38.1 g/mol Answer: E

Calculate the molar mass of a gas that has a density of 1 Calculate the molar mass of a gas that has a density of 1.70 g/L at STP. A. 2.02 g/mol B. 4.00 g/mol C. 28.0 g/mol D. 32.0 g/mol E. 38.1 g/mol Answer: E

The partial pressures in a mixture of CO2, N2, and O2 in a sample of gas are 50.0 atm, 495 atm, and 205 atm, respectively. Calculate the mole percentage of each gas. A. 5.00%, 70.3%, 24.7% B. 6.67%, 66.0%, 27.3% C. 0.500%, 49.5%, 50.0% D. 10.0%, 50.0%, 40.0% E. 1.50%, 75.5%, 23.0% Answer: B

The partial pressures in a mixture of CO2, N2, and O2 in a sample of gas are 50.0 atm, 495 atm, and 205 atm, respectively. Calculate the mole percentage of each gas. A. 5.00%, 70.3%, 24.7% B. 6.67%, 66.0%, 27.3% C. 0.500%, 49.5%, 50.0% D. 10.0%, 50.0%, 40.0% E. 1.50%, 75.5%, 23.0% Answer: B

A sample of hydrogen gas is collected over water at a pressure of 635 mm Hg at 10.0 °C. Calculate the partial pressure of hydrogen. (The vapor pressure of water at 10.0 °C is 9.2 mm Hg.) A. 9 mm Hg B. 69 mm Hg C. 626 mm Hg D. 635 mm Hg E. 644 mm Hg Answer: C

A sample of hydrogen gas is collected over water at a pressure of 635 mm Hg at 10.0 °C. Calculate the partial pressure of hydrogen. (The vapor pressure of water at 10.0 °C is 9.2 mm Hg.) A. 9 mm Hg B. 69 mm Hg C. 626 mm Hg D. 635 mm Hg E. 644 mm Hg Answer: C

How many liters of oxygen gas are produced by the complete decomposition of 225 mL of water? The oxygen gas is collected at 580. torr and 27 °C. (The density of water at 27 °C is 1.00 g/mL) A. 0.225 L B. 36.3 L C. 201 L D. 403 L E. 0.0239 L Answer: C

How many liters of oxygen gas are produced by the complete decomposition of 225 mL of water? The oxygen gas is collected at 580. torr and 27 °C. (The density of water at 27 °C is 1.00 g/mL) A. 0.225 L B. 36.3 L C. 201 L D. 403 L E. 0.0239 L Answer: C

How many grams of water are produced from the complete combustion of 15.8 L of propane (C3H8) gas at STP? A. 0.705 g B. 2.82 g C. 12.7 g D. 38.1 g E. 50.8 g Answer: E

How many grams of water are produced from the complete combustion of 15.8 L of propane (C3H8) gas at STP? A. 0.705 g B. 2.82 g C. 12.7 g D. 38.1 g E. 50.8 g Answer: E

Which of the following samples occupy the largest volume at STP? A. 1.00 mol O2 B. 48.0 g O2 C. 0.500 mol He D. 4.008 g H2 E. 6.02 × 1023 molecules of N2 Answer: D

Which of the following samples occupy the largest volume at STP? A. 1.00 mol O2 B. 48.0 g O2 C. 0.500 mol He D. 4.008 g H2 E. 6.02 × 1023 molecules of N2 Answer: D

For an ideal gas, which two variables are inversely proportional to each other, assuming all the other conditions remain constant? A. V and P B. T and P C. V and T D. V and n E. None of the above Answer: A

For an ideal gas, which two variables are inversely proportional to each other, assuming all the other conditions remain constant? A. V and P B. T and P C. V and T D. V and n E. None of the above Answer: A

A. increases by a factor of 75. B. halves. C. doubles. At a constant pressure, when the temperature of a gas sample is doubled from 75 °C to 150 °C, the volume of the gas A. increases by a factor of 75. B. halves. C. doubles. D. remains the same. E. None of the above Answer: C

A. increases by a factor of 75. B. halves. C. doubles. At a constant pressure, when the temperature of a gas sample is doubled from 75 °C to 150 °C, the volume of the gas A. increases by a factor of 75. B. halves. C. doubles. D. remains the same. E. None of the above Answer: C

Which of the following gas laws relate volume and temperature? A. Avogadro’s law B. Boyle’s law C. Charles’s law D. Gay-Lussac’s law E. Dalton’s Law Answer: C

Which of the following gas laws relate volume and temperature? A. Avogadro’s law B. Boyle’s law C. Charles’s law D. Gay-Lussac’s law E. Dalton’s Law

What is the SI unit for pressure? A. Pa B. atm C. mm Hg D. torr E. psi Answer: A

What is the SI unit for pressure? A. Pa B. atm C. mm Hg D. torr E. psi Answer: A

A 158 mL sample of gas has a pressure of 0 A 158 mL sample of gas has a pressure of 0.989 atm and a temperature of 25.0 °C. What is the final temperature (°C) when the pressure increases to 1.01 atm and the volume decreases to 192 mL? A. 369 °C B. 25.0 °C C. 96.8 °C D. 2.47 °C E. 9.68 °C Answer: C

A 158 mL sample of gas has a pressure of 0 A 158 mL sample of gas has a pressure of 0.989 atm and a temperature of 25.0 °C. What is the final temperature (°C) when the pressure increases to 1.01 atm and the volume decreases to 192 mL? A. 369 °C B. 25.0 °C C. 96.8 °C D. 2.47 °C E. 9.68 °C Answer: C

If a 7. 45 L sample of nitrogen at STP is compressed to a volume of 5 If a 7.45 L sample of nitrogen at STP is compressed to a volume of 5.81 L and warmed to 295 K, what is the final pressure of the sample? A. 1.38 atm B. 8.85 atm C. 5.68 atm D. 0.989 atm E. 1.27 atm Answer: C

If a 7. 45 L sample of nitrogen at STP is compressed to a volume of 5 If a 7.45 L sample of nitrogen at STP is compressed to a volume of 5.81 L and warmed to 295 K, what is the final pressure of the sample? A. 1.38 atm B. 8.85 atm C. 5.68 atm D. 0.989 atm E. 1.27 atm Answer: C

A mixture of nitrogen, hydrogen, and oxygen has a total pressure of 695 mm Hg. If the partial pressure of nitrogen is 435 mm Hg and the partial pressure of hydrogen is 205 mm Hg, what is the partial pressure of oxygen? A. 0.072 atm B. 695 mm Hg C. 125 mm Hg D. 55 mm Hg E. Two of the above Answer: E

A mixture of nitrogen, hydrogen, and oxygen has a total pressure of 695 mm Hg. If the partial pressure of nitrogen is 435 mm Hg and the partial pressure of hydrogen is 205 mm Hg, what is the partial pressure of oxygen? A. 0.072 atm B. 695 mm Hg C. 125 mm Hg D. 55 mm Hg E. Two of the above Answer: E

Water decomposes to form hydrogen and oxygen gases Water decomposes to form hydrogen and oxygen gases. What volume of oxygen gas measured at 750 mm Hg and 35 °C is formed when 28 g of water is reacted? A. 22.4 L B. 45 L C. 720 mL D. 130 mL E. 20. L Answer: E

Water decomposes to form hydrogen and oxygen gases Water decomposes to form hydrogen and oxygen gases. What volume of oxygen gas measured at 750 mm Hg and 35 °C is formed when 28 g of water is reacted? A. 22.4 L B. 45 L C. 720 mL D. 130 mL E. 20. L Answer: E

What is the mass of a sample of chlorine gas that occupies a volume of 2.500 L at STP? A. 0.1115 g B. 7.9 g C. 1.295 g D. 7.904 g E. 3.953 g Answer: D

What is the mass of a sample of chlorine gas that occupies a volume of 2.500 L at STP? A. 0.1115 g B. 7.9 g C. 1.295 g D. 7.904 g E. 3.953 g Answer: D