Question

GAS LAW PROBLEMS 1. What volume will 500 mL of gas at 20 °C and a pressure of 420 mm Hg occupy if the temperature is reduced to -80 °C and the pressure is increased to 650 mm Hg? 2. A sample of gas of mass 2.82 g occupies a volume of 639 mL at 27 °C and 1.00 atm pressure. What is the molar mass of the gas? 3. A gas is placed in a storage tank at a pressure of 30.0 atm at 20.3 °C. As a safety device, a small metal plug in the tank is made of a metal alloy that melts at 130 °C. If the tank is heated, what is the maximum pressure that will be attained in the tank before the plug melts and releases gas? 4. Forty liters (40 L) of a gas were collected over water when the barometer read 622.0 mm Hg and the temperature was 20 °C. What volume would the dry gas occupy at standard conditions? [HINT: Consider Dalton's law of partial pressures.] 5. Five moles (5.0 mol) of hydrogen gas at 0 °C are forced into a steel cylinder with a volume of 2.0 L. What is the pressure of the gas, in mm Hg, in the cylinder? 6. What is the density of He at STP? Why do helium-filled balloons rise in air?

          GAS LAW PROBLEMS
1. What volume will 500 mL of gas at 20 °C and a pressure of 420 mm Hg occupy if the temperature is reduced to -80 °C and the pressure is increased to 650 mm Hg?
2. A sample of gas of mass 2.82 g occupies a volume of 639 mL at 27 °C and 1.00 atm pressure. What is the molar mass of the gas?
3. A gas is placed in a storage tank at a pressure of 30.0 atm at 20.3 °C. As a safety device, a small metal plug in the tank is made of a metal alloy that melts at 130 °C. If the tank is heated, what is the maximum pressure that will be attained in the tank before the plug melts and releases gas?
4. Forty liters (40 L) of a gas were collected over water when the barometer read 622.0 mm Hg and the temperature was 20 °C. What volume would the dry gas occupy at standard conditions? [HINT: Consider Dalton's law of partial pressures.]
5. Five moles (5.0 mol) of hydrogen gas at 0 °C are forced into a steel cylinder with a volume of 2.0 L. What is the pressure of the gas, in mm Hg, in the cylinder?
6. What is the density of He at STP? Why do helium-filled balloons rise in air?

GAS LAW PROBLEMS
1. What volume will 500 mL of gas at 20 °C and a pressure of 420 mm Hg occupy if the temperature is reduced to -80 °C and the pressure is increased to 650 mm Hg?
2. A sample of gas of mass 2.82 g occupies a volume of 639 mL at 27 °C and 1.00 atm pressure. What is the molar mass of the gas?
3. A gas is placed in a storage tank at a pressure of 30.0 atm at 20.3 °C. As a safety device, a small metal plug in the tank is made of a metal alloy that melts at 130 °C. If the tank is heated, what is the maximum pressure that will be attained in the tank before the plug melts and releases gas?
4. Forty liters (40 L) of a gas were collected over water when the barometer read 622.0 mm Hg and the temperature was 20 °C. What volume would the dry gas occupy at standard conditions? [HINT: Consider Dalton's law of partial pressures.]
5. Five moles (5.0 mol) of hydrogen gas at 0 °C are forced into a steel cylinder with a volume of 2.0 L. What is the pressure of the gas, in mm Hg, in the cylinder?
6. What is the density of He at STP? Why do helium-filled balloons rise in air?

Added by Melanie F.

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