Quiz #3-5 PRACTICE: Combined & Ideal Gas Laws
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If a sample of gas occupies 6.8 L at 376°C and 1.5 atm, what will be its volume at standard temperature and pressure (STP)?
Which of the following accurately describes the particles of an ideal gas?
particles have no mass or volume
particles are affected by intermolecular forces at extremely high pressures
particles can undergo chemical reactions
particles will condense to a liquid when compressed and/or cooled
A sample of 2.35 moles of helium gas occupies 57.9 L at 27.0°C and 1.00 atm. At 150.°C and 1.00 atm, the volume of this sample is:
The amount of neon gas that occupies 60.82 L at 31°C and 48.9 kPa is:
What is the volume occupied by 5.29 mol of a gas at 44°C and 105.7 kPa?
A container with an initial volume of 1.00 L is occupied by a gas at a pressure of 155 kPa at 25°C. By changing the pressure, the volume of the gas increases to 6.00 L as the temperature is simultaneously raised to 100.°C. What is the new pressure of the container?
A sample of a gas originally at 25°C and 1.00 atm pressure in a 2.5 L container is allowed to expand until the pressure is 0.85 atm and the temperature is 15°C. The final volume of the gas is:
A gas occupies 355 mL at a pressure of 99.5 kPa and a temperature of 22°C. The pressure on the gas is subsequently increased by 10.0 kPa and the volume is dropped by 75 mL. What is the new temperature?
The pressure of a sample of 6.022 g CH4 in a 30.0 L vessel at 402 K is:
A 0.325 L flask filled with gas at 0.914 atm and 19°C contains:
1.22 x 10-4 mol
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