1. Calculate the temperature of 4.00 moles of ideal gas at a pressure of 2.00 atm and a volume
of 54.0 L. (Use 0.0821 L. atm/mol. Kas the gas constant.)
2. Determine what happens to the pressure of the above sample of ideal gas if the volume
is halved and the temperature doubles.
A student states that if the volume of a sample of ideal gas increases to three times the original
volume, and the pressure also increases to three times the original pressure, the temperature of the
gas will remain unchanged.
3. Explain why the student is incorrect.
4. Determine the actual temperature of the ideal gas.
A. Calculate the temperature of 4.00 moles of ideal gas at a pressure of 2.00
atm and a volume of 54.0 L. (Use 0.0821 L. atm/mol · K as the gas
constant.)
Answers: 2
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