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

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

The ** pressure, volume, and temperature of a gas** are related to the number of moles of gas and the universal gas constant:

$\frac{\mathbf{PV}}{\mathbf{T}}\mathbf{=}\mathbf{nR}$

The value **nR is constant**. For a given mole of gas, the initial and final pressure, volume, and temperature of the gas are related by the ** combined gas law**:

$\overline{)\frac{{\mathbf{P}}_{\mathbf{1}}{\mathbf{V}}_{\mathbf{1}}}{{\mathbf{T}}_{\mathbf{1}}}{\mathbf{=}}\frac{{\mathbf{P}}_{\mathbf{2}}{\mathbf{V}}_{\mathbf{2}}}{{\mathbf{T}}_{\mathbf{2}}}}$

**Solve for ****T**_{2}**:**

What is the temperature of an 11.2-L sample of carbon monoxide, CO, at 744 torr if it occupies 13.3 L at 55 °C and 744 torr?

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Our tutors have indicated that to solve this problem you will need to apply the Chemistry Gas Laws: Combined Gas Law concept. You can view video lessons to learn Chemistry Gas Laws: Combined Gas Law. Or if you need more Chemistry Gas Laws: Combined Gas Law practice, you can also practice Chemistry Gas Laws: Combined Gas Law practice problems.

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