Consider two identical sealed containers containing N2 (g) at 273 K. One container contains 1 mol of N2 (g) and the other 4 mols of N2 (g).
Which of the following statements is true?
The pressure is greater in vessel 1.
The force at which the molecules collide with the walls is greater in vessel 1 than vessel 2.
The pressure is the same in each vessel.
The average kinetic energy of the molecules is the same in both vessels.
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The distribution of molecular energies in a sample of a gas at a given temperature is shown by the Boltzmann distribution graph above.
If the temperature is increased, what will happen to the position of point X?
Fewer molecules possess the most probable energy value so X will shift to the right.
Fewer molecules possess the most probable energy value so X will shift to the left.
More molecules possess the most probable energy value so X will shift to the left.
The position of X will stay the same but the area under the distribution curve increases.
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For an ideal gas at constant pressure and temperature, which diagram shows the correct graph of pV against n?
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An experiment is conducted to calculate the molar mass of an unknown gas of known mass.
Measurements of pressure, volume and temperature are taken during the experiment.
Which conditions of temperature and pressure would give the most accurate value of molar mass?
low pressure, high tempearture
low pressure, low temperature
high pressure, high temperature
high pressure, low temperature
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1 mark0.96 g of hydrogen gas is contained in a sealed vessel of volume of 7.0 L at a temperature of 303 K.
What is the pressure of the vessel?
0.48 atm
1.69 atm
3.27 atm
0.59 atm
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1 markA sample of chlorine gas with a of mass 5.35 g has a volume of 1.25 L at a pressure of 1.00 atm. What is the temperature of the gas?
4.92 x 10-3 K
2.85 K
81.0 K
203 K
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1 L of gas X and 1 L of gas Y are kept at the same temperature and pressure.
The speed of the molecules is plotted against the fraction of molecules with that speed. What can be deduced about the two gases?
The molar mass of X is larger than the molar mass of Y.
The molar mass of Y is larger than the molar mass of X.
The average kinetic energy of X is higher than that of Y.
The average kinetic energy of Y is higher than that of X.
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Which graph shows how the average kinetic energy of a gas varies with temperature?
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1 markA mixture of three gases in a sealed container is able to generate 4.5 atm of pressure. The identities and amounts of each gas are as follows:
0.3 moles of Cl2, 0.4 moles of N2, 0.5 moles of Ar.
What is the partial pressure of nitrogen gas?
1.125 atm
1.50 atm
1.20 atm
1.875 atm
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1 markA sealed 6.00 L cylinder contains 13.30 g of CO2 (g) and 17.00 g of Ar (g).
What is the total pressure, in atm, of the gas mixture in the cylinder at 303 K?
125.6 atm
1.24 atm
3.03 atm
1.78 atm
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1 mark
The glass containers X and Y are connected by a closed valve.
X contains pure CO2 gas at 298 K and a pressure of 1.00 atm. Container Y has been evacuated prior to the experiment and has a volume three times bigger than container X.
During the experiment, the valve is opened, and the temperature of the whole apparatus is raised to 433 K.
What is the final pressure in the system?
0.36 atm
2.75 atm
0.48 atm
2.06 atm
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A sample of bromine and nitrogen gas in a closed container of constant volume is cooled until its absolute temperature is halved.
Which of the following statements is true?
The average speed of the gas molecules remains the same.
The number of molecules per L of bromine gas will decrease.
The volume of the gases will halve.
The density of the gases will decrease.
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Which of the following best explains why CO2 deviates from ideal gas behavior at a low temperature and high pressure?
CO2 molecules move too quickly to interact with each other
CO2 molecules have significant intermolecular attractions, causing the measured pressure to be lower than predicted
The volume of CO2 molecules becomes negligible
CO2 collisions with container walls are perfectly elastic, as assumed in ideal gases
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A gas mixture at equilibrium held over water at 35°C contains 3.0 moles of helium, 5.0 moles of argon, and 2.0 moles of water vapor.
If the total pressure exerted by the gases is 740 mmHg, what is the vapor pressure of water at 35°C?
100 mmHg
200 mmHg
148 mmHg
592 mmHg
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A 4.5 L container holds ethane gas at 50°C and a pressure of 3.5 atm.
If the temperature is increased to 350°C and the pressure is reduced to 1.5 atm, what is the final volume of the gas?
10.5 L
15.2 L
20.3 L
25.6 L
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