We’re asked to **determine ****what happens to the temperature** of a **fixed amount of an ideal gas** at a *constant volume* when its **pressure is doubled**.

Recall that the ** ideal gas law** is:

$\overline{){\mathbf{PV}}{\mathbf{=}}{\mathbf{nRT}}}$

The ** pressure and temperature of a gas** are related to the number of moles, gas constant and temperature. The value

$\overline{)\frac{\mathbf{P}}{\mathbf{T}}{\mathbf{=}}\frac{\mathbf{nR}}{\mathbf{V}}}$

Suppose you have a fixed amount of an ideal gas at a constant volume.

If the pressure of the gas is doubled while the volume is held constant, what happens to its temperature? [Section 10.4]

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