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- 1. Multiple ChoiceDalton's Law states...that at a constant temperature the volume of a confined ideal gas varies inversely with its pressure.that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gaseshow gases tend to expand when heatedthat the density of an ideal gas at constant pressure varies inversely with the absolute temperature of the gas.
- 2. Multiple Choice
Which equation represents Dalton's Law?e=mc2PV=nRTP1/T1=P2/T2Ptotal=P1, P2, P3... - 3. Multiple ChoiceDalton's law of...Partial PressureThermodynamicsIdeal GasPhysics
- 4. Multiple ChoiceThree gases, Ar, N2 and H2 are mixed in a 500L container. Ar has a pressure of 255 torr, N2 has a pressure of 228torr and H2 has pressure of 752torr. What is the total pressure in the container?483torr270torr1235torr
- 5. Multiple ChoiceCalculate the partial pressure of H2 at 20oC when the vapor pressure of water is 17.5torr. The total pressure of the gases is 750torr.767.5torr732torr42.86torr
- 6. Multiple ChoiceA mixture of hydrogen, nitrogen, and water vapor has a total pressure of 864 mmHg. The partial pressure of hydrogen is 220 mmHg and that of nitrogen is 410 mmHg. What is the partial pressure of water vapor?234 mmHg1.37 mmHg2.64 mmHg1, 494 mmHg
- 7. Multiple Choice
A container holds a mixture of two different gases. The oxygen in a container exerts 80 mmHg of pressure on the inside of the container. The total pressure inside the container is 120 mmHg. What is the pressure of the other gas in the container?
200 mmHg
80 mmHg
40 mmHg
120 mmHg
- 8. Multiple Choice
A container contains three gases, N2, O2 and Ar, with partial pressures of 23.3 kPa, 40.9 kPa and 13.7 kPa respectively. What is the total pressure inside the container?
64.5 kPa
77.9 kPa
63.4 kPa
10.4 kPa
- 9. Multiple Choice
In the chem lab, a student filled a balloon with 2 different gases, CO2 and N2. The atmospheric pressure in the chem lab was 770.0 mmHg and the partial pressure of CO2 added to the balloon was 0.3255 atm. What was the partial pressure of N2 in the balloon?
522.6 mmHg
5.226 mmHg
773.5 mmHg
205.36 mmHg
- 10. Multiple Choice
A container holds three gases: oxygen, carbon dioxide, and helium. The partial pressures of the three gases are 2.00 atm, 3.00 atm, and 4.00 atm, respectively. What is the total pressure inside the container?
900 atm
0.90 atm
9.00 atm
920 atm
- 11. Multiple ChoiceThe rate of effusion is _______________ proportional to the square root of its' molar mass.DirectlyInversely
- 12. Multiple ChoiceLighter gases have a ________________ rate of effusion.fasterslowerrate of effusion does not depend on mass.
- 13. Multiple ChoiceWhich of the following would have a faster rate of effusion: 15g of Kr or 15g of N2?KyrptonNitrogenBoth would have the same rate of effusion
- 14. Multiple ChoiceEffusion isused to describe the combustibility of a gas.ability of a gas to escape through a tiny openingwhat occurs after diffusion.the ability of a gas to mix with other gases.
- 15. Multiple ChoiceThe rate of effusion of water vapor is 0.391 and the rate of effusion of propane is 0.251 at the same temperature and pressure. What is the molar mass of propane? (write the formula and show your work)44.0 g/mol6.63 g/mol0.37 g/mol28.2 g/mol
- 16. Multiple Choice
Identify the factor that determines rates of diffusion and effusion for different molecules at a given temperature.
Size of the molecules
Polarity of the molecules
Temperature of the gas
Molar mass of the gas
- 17. Multiple Choice
Effusion and diffusion rates are inversely proportional to the square root of the molar mass of the gas.
True
False
- 18. Multiple Choice
Why would O2 effuse faster than CO2 in the same room
because it has more energy
because it has a greater molar mass
because oxygen has a higher temperature
they will effuse the same because the temperature is fixed
- 19. Multiple ChoiceWhich of the following gases will effuse most slowly under the same physical conditions?
Don't forget to check for diatomics!HydrogenChlorineAmmonia (NH3)Bromine - 20. Multiple ChoiceUse Graham’s Law to calculate fast O2 gas will effuse compared to Cl2.O2 effuses 1.5x faster than Cl2O2 effuses 0.11x as fast as Cl2O2 effuses 1.1x faster than Cl2O2 effuses 0.15x as fast as Cl2
- 21. Multiple ChoiceCalculate the relative rate of effusion of gaseous oxygen and nitrogen.4.001.073.740.94
- 22. Multiple ChoiceHow much faster will gaseous hydrogen effuse than gaseous chlorine under the same physical conditions?5.925.950.031.00
- 23. Multiple ChoiceEffusion isused to describe the combustibility of a gas.the ability of a gas to move from a high pressure to a low pressurewhat occurs after diffusion.the ability of a gas to mix with other gases.
- 24. Multiple ChoiceThe rate of effusion is _______________ proportional to the square root of its' molar mass.DirectlyInversely
- 25. Multiple ChoiceHeavier gases have a __________________ rate of effusion.FasterSlowerRate of effusion does not depend on mass.
- 26. Multiple ChoiceWhich of the following would have a faster rate of effusion: 12 mol of Chlorine or 10 mol of Helium?12 mol of Chlorine10 mol of Helium
- 27. Multiple ChoiceAn unknown gas diffuses 0.25 times as fast as helium gas (He). What is the molecular mass of the unknown gas?64 g/mol16 g/mol32 g/mol4 g/mol
- 28. Multiple ChoiceUnder the same conditions, how many times faster will hydrogen gas effuse than carbon dioxide gas?4.694.580.2180.213
- 29. Multiple Choice
How many times faster does He effuse compared to N2 (He = 4 N2 = 28)
1.2 times faster
2.65 times faster
7 times faster
0.377 times faster
- 30. Multiple ChoiceWhich is the correct equation for Dalton's law representing a mixture o three gasesPT = P1 - P2 - P3PT = P1 + P2 - P3P1 = PT - P2 - P3
- Answer choicesTagsAnswer choicesTags