Initially, a gas sample has a volume of 2.00 L at 27 ˚C and 1.00 atm. We’re being asked to determine the temperature of the gas if the pressure changes to 1.25 atm and the volume changes to 3.00 L.
Recall that the ideal gas law is:
The pressure, volume, and temperature of a gas are related to the number of moles of gas and the universal gas constant:
The value nR is constant. For a given moles of gas, the initial and final pressure, volume, and temperature of the gas are related by the combined gas law:
If you have 2.00 L of a gas initially at 1.00 atm and 27 °C, what temperature will it have at 3.00 L and 1.25 atm?
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