Have an account?
Skip to Content
Build your own quiz
20 questions
Show Answers
See Preview
- 1. Multiple Choice
Consider the two samples of helium gas pictured. The gases are in a flexible container. Which of the following best explains the differences in volume of the two samples? Justify your answer.The Kelvin temperature of container B is triple the Kelvin temperature of container A. According to the equation PV=nRT, volume and Kelvin temperature are INVERSELY related. If the Kelvin temp is tripled under constant pressure and number of moles conditions, the volume must triple as well.The Kelvin temperature of container A is triple the Kelvin temperature of container B. According to the equation PV=nRT, volume and Kelvin temperature are DIRECTLY related. If the Kelvin temp is tripled under constant pressure and number of moles conditions, the volume must triple as well.The Kelvin temperature of container B is triple the Kelvin temperature of container A. According to the equation PV=nRT, volume and Kelvin temperature are DIRECTLY related. If the Kelvin temp is tripled under constant pressure and number of moles conditions, the volume must triple as well.The Kelvin temperature of container A is triple the Kelvin temperature of container B. According to the equation PV=nRT, volume and Kelvin temperature are INVERSELY related. If the Kelvin temp is tripled under constant pressure and number of moles conditions, the volume must triple as well. - 2. Multiple ChoiceConsider the two samples of helium gas pictured. The gases are in a flexible container. Which of the following best explains the differences in pressure of the two samples? Justify your answer.The volume of container B is double the volume of container A. According to the equation PV=nRT, pressure and volume are DIRECTLY related. If the volume is doubled under constant temperature and number of moles conditions, pressure will be halved.The volume of container B is double the volume of container A. According to the equation PV=nRT, pressure and volume are INVERSELY related. If the volume is doubled under constant temperature and number of moles conditions, pressure will be halved.The volume of container A is double the volume of container B. According to the equation PV=nRT, pressure and volume are INVERSELY related. If the volume is doubled under constant temperature and number of moles conditions, pressure will be halved.The volume of container A is double the volume of container B. According to the equation PV=nRT, pressure and volume are DIRECTLY related. If the volume is doubled under constant temperature and number of moles conditions, pressure will be halved.
- 3. Multiple ChoiceConsider the two samples of helium gas pictured. The samples are in a rigid container. Which of the following best explains the differences in pressure of the two samples? Justify your answer.The number of moles of He in container B is double the number of moles of container A. According to the equation PV=nRT, pressure and number of moles are DIRECTLY related. If the pressure is doubled under constant temperature and volume conditions, the number of moles will double as well.The number of moles of He in container B is double the number of moles of container A. According to the equation PV=nRT, pressure and number of moles are INVERSELY related. If the pressure is doubled under constant temperature and volume conditions, the number of moles will double as well.The number of moles of He in container A is double the number of moles of container B. According to the equation PV=nRT, pressure and number of moles are DIRECTLY related. If the pressure is doubled under constant temperature and volume conditions, the number of moles will double as well.The number of moles of He in container A is double the number of moles of container B. According to the equation PV=nRT, pressure and number of moles are INVERSELY related. If the pressure is doubled under constant temperature and volume conditions, the number of moles will double as well.
- 4. Multiple ChoiceHow does the average kinetic energy of the helium atoms in Container A compare to the average kinetic energy of the helium atoms in Container B?The average kinetic energy of helium atoms in Container A is half the average kinetic energy of helium atoms in Container B because the pressure in Container A is half the pressure in Container B. Average kinetic energy is directly related to pressure.The average kinetic energy of helium atoms in Container A is half the average kinetic energy of helium atoms in Container B because the number of moles in Container A is half the number of moles in Container B. Average kinetic energy is directly related to number of moles.The average kinetic energy of helium atoms in Container A is the same as the average kinetic energy of helium atoms in Container B because the volumes of the containers are the same. Average kinetic energy is directly related to volume.The average kinetic energy of helium atoms in Container A is the same as the average kinetic energy of helium atoms in Container B because the temperatures of the gases in the containers are the same. Average kinetic energy is directly related to temperature.
- 5. Multiple ChoiceConsider the mixture of gases pictured.
Helium has the _________ AVERAGE KINETIC ENERGY as neon because it has _____________.SAME:
THE SAME TEMPERATURESAME:
THE SAME PRESSUREHIGHER:
THE LOWER MOLAR MASSLOWER:
THE HIGHER MOLAR MASS - 6. Multiple ChoiceConsider the mixture of gases pictured.
Which of the gases occupy a larger volume?Helium because it has a smaller molar mass.Neon because it has a larger molar mass.The both occupy the same volume because they are in the same container.It is impossible to tell without knowing the number of moles of each gas. - 7. Multiple ChoiceConsider the mixture of gases pictured.
Helium has the _________ VELOCITY as neon because it has _____________.SAME:
THE SAME TEMPERATURESAME:
THE SAME PRESSUREHIGHER:
THE LOWER MOLAR MASSLOWER:
THE HIGHER MOLAR MASS - 8. Multiple ChoiceThe following plot is for an ideal gas. Consider the ideal gas equation, PV=nRT, and identify what state function(s) could be represented by x for this plot.P, T, or nP, or TP, or nT, or n
- 9. Multiple ChoiceA rigid vessel is connected to four separate 2.00 liter gas cylinders. Each cylinder contains a separate, diatomic gas at room temperature. When the gases are combined and held at room temperature, which of the following most accurately describes what happens in the reaction vessel?All of the gases immediately diffuse at the same rate, causing the kinetic energy of the substances to increase.The heavier diatomic gases diffuse slower than the lighter diatomic gases, causing a heterogeneous mixture in the new system.The rate of diffusion differs for each gas, but the overall kinetic energy of the system remains constant.The lightest mass gas is unable to diffuse into the new system due to the increased pressure by the heavier gases causing only three of the four gases to mix in the new container.
- 10. Multiple ChoiceThe N2 gas particles in the container shown is initially at 27°C. The lengths of the arrows represents the speeds of the particles. Which of the following diagrams best represents the particles when the vessel is heated to 127°C?ABCD
- 11. Multiple ChoiceBased on the Maxwell-Boltzmann distribution of the fraction of molecules in a gas sample plotted against the molecular speed of the molecules, which of the following statements does NOT relate to the data presented?The hydrogen gas has the fastest speed due to the low molecular mass of the gas.Polarity of a gas does not affect the average molecular speed of the gas in the mixture.Oxygen has the highest fraction of molecules overall in the gas mixture.Water must be in the vapor phase not the liquid phase for this particular graph.
- 12. Multiple ChoiceBased on the following information, which gas would have the highest average particle velocity when all gases are placed in a rigid container?Carbon dioxideEthaneAmmoniaAll would have the same average particle velocity because they are at the same temperature.
- 13. Multiple ChoiceThree gases are placed into separate isolated rigid containers under the conditions indicated in the table. Which of the following statements indicates which pure sample of gas has the highest average kinetic energy?The nitrogen gas would have the greatest kinetic energy due to the larger molar mass.The hydrogen gas would have the highest kinetic energy due to the highest root mean square velocity based on the lowest molar mass.The ammonia gas would have the highest kinetic energy due to the polar nature of the gas.The kinetic energy of the three gases would be the same because they are all at the same temperature.
- 14. Multiple ChoiceWhich statement is TRUE about kinetic molecular theory?A single particle does not move in a straight line.The size of the particle is large compared to the volume.The collisions of particles with one another is completely elastic.The average kinetic energy of a particle is not proportional to the temperature.
- 15. Multiple ChoiceA vessel at 987 mmHg contains nitrogen, argon, helium, and carbon dioxide gases. The partial pressure of the first three gases are 44.0 mmHg, 466 mmHg, and 220 mmHg respectively. What is the partial pressure of carbon dioxide in atm?1.30 atm2.00 atm0.338 atm0.961 atm
- 16. Multiple ChoiceIdentify the correct statement regarding the Kinetic Molecular Theory.As temperature decreases, this causes velocity to decrease.Gas particles are closely associated with each other.Intermolecular forces are strong.Collisions are effective (inelastic).
- 17. Multiple ChoiceA gas has a pressure of 2.26 atm and occupies a volume of 4.40 L. If the gas is compressed to a volume of 2.68 L, what will its pressure be, assuming constant temperature?3.71atm1.38atm5.22atm2.68atm
- 18. Multiple ChoiceAt standard temperature, a gas has a volume of 332 mL. The temperature is then increased to 128°C, and the pressure is held constant. What is the new volume?Unable to determine without initial temperature.226mL488mL708mL
- 19. Multiple ChoiceA sample of gas is collected over water at a temperature of 35.0°C when the barometric pressure reading is 618.0 torr. What is the partial pressure of the dry gas, given PH2O = 42.2 torr?575.8torr660.2torr308.0torr653.0torr
- 20. Multiple ChoiceA sample of ideal gas occupies 250. mL at 25.0°C and 740.mmHg. What is its volume at STP?2660mL223mL594mL1,320mL
- Answer choicesTagsAnswer choicesTags