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A gas mixture with a total pressure of 745mmHg contains each of the following gases at the indicated partial pressures: CO2, 125 mmHg; Ar, 214 mmHg; and O2, 187 mmHg. The mixture also contains helium gas. What is the partial pressure of the helium gas? What mass of helium gas is present in a 12.0-L sample of this mixture at 273 K? 

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A sample of gas has a mass of 0.555 g. Its volume is 117 ml at a temperature of 85 °C and a pressure of 753 mmHg. Find the molar mass of the gas. 

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An experiment shows that a 113-mL gas sample has a mass of 0.171 g at a pressure of 721 mmHg and a temperature of 32°C. What is the molar mass of the gas? 

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A sample of N2O gas has a density of 2.85 g/L at 298 K. What is the pressure of the gas (in mmHg)? 

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Use the molar volume of a gas at STP to calculate the density (in g/L) of nitrogen gas at STP. 

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Use the molar volume of a gas at STP to determine the volume (in L) occupied by 33.6 g of neon at STP. 

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A sample of nitrogen gas in a 1.75-L container exerts a pressure of 1.35 atm at 25 °C. What is the pressure if the volume of the container is maintained constant and the temperature is raised to 355 °C? 

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This picture represents a sample of gas at a pressure of 1 atm, a volume of 1 L, and a temperature of 25 °C. Draw a similar picture showing what would happen to the sample if the volume were reduced to 0.5 L and the temperature increased to 250 °C. What would happen to the pressure? 

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Which gas sample representation has the greatest pressure? Assume that all the samples are at the same temperature. Explain 

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Pressurized carbon dioxide inflators can be used to inflate a bicycle tire in the event of a flat. These inflators use metal cartridges that contain 16.0 g of carbon dioxide. At 298 K, to what pressure (in psi) can the carbon dioxide in the cartridge inflate a 3.45-L mountain bike tire? (Note: The gauge pressure is the difference between the total pressure and atmospheric pressure. In this case, assume that atmospheric pressure is 14.7 psi.) 

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A 1.0-L container of liquid nitrogen is kept in a closet measuring 1.0 m by 1.0 m by 2.0 m. Assuming that the container is completely full, that the temperature is 25.0 °C, and that the atmospheric pressure is 1.0 atm, calculate the percent (by volume) of air that is displaced if all of the liquid nitrogen evaporates. (Liquid nitrogen has a density of 0.807 g/mL.) 

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A weather balloon is inflated to a volume of 28.5 L at a pressure of 748 mmHg and a temperature of 28.0 °C. The balloon rises in the atmosphere to an altitude of approximately 25,000 feet, where the pressure is 385 mmHg and the temperature is -15.0 °C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude. 

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What is the temperature of 0.52 mol of gas at a pressure of 1.3 atm and a volume of 11.8 L? 

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What is the pressure in a 15.0-L cylinder filled with 32.7 g of oxygen gas at a temperature of 302 K? 

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What is the volume occupied by 12.5 g of argon gas at a pressure of 1.05 atm and a temperature of 322 K? Would the volume be different if the sample were 12.5 g of helium (under identical conditions)? 

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A cylinder with a moveable piston contains 0.553 mol of gas and has a volume of 253 mL. What will its volume be if an additional 0.365 mol of gas is added to the cylinder? (Assume constant temperature and pressure.) 

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A syringe containing 1.55 mL of oxygen gas is cooled from 95.3°C to 0.0°C. What is the final volume of oxygen gas? 

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A sample of gas has an initial volume of 13.9 L at a pressure of 1.22 atm. If the sample is compressed to a volume of 10.3 L, what is its pressure? 

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Given a barometric pressure of 751.5 mmHg, calculate the pressure of each gas sample as indicated by the manometer. 

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Given a barometric pressure of75 1.5 mmHg, calculate the pressure of each gas sample as indicated by the manometer. 

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The world record for lowest pressure (at sea level) was 652.5 mmHg recorded inside Typhoon Tip on October 12,1979, in the Western Pacific Ocean. Convert this pressure to 

d. psi

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The world record for lowest pressure (at sea level) was 652.5 mmHg recorded inside Typhoon Tip on October 12,1979, in the Western Pacifie Ocean. Convert this pressure to 

c. in Hg

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The world record for lowest pressure (at sea level) was 652.5 mmHg recorded inside Typhoon Tip on October 12, 1979, in the Western Pacifie Ocean. Convert this pressure to 

b. atm

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The pressure on top of Mt. Everest averages about 235 mmHg. Convert this pressure to

d. atm

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The pressure on top of Mt. Everest averages about 235 mmHg. Convert this pressure to

c. in Hg

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