Initially, a gas in a closed container has a temperature of 30°C and a pressure of 760 mm Hg. We’re being asked to determine the **pressure of the gas sample **if the temperature changes to 1155°C.

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 moles of gas, the initial and final pressure, volume, and temperature of the gas are related by the * combined gas law*:

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

Since the container is closed, the **volume of the gas remains constant** and the combined gas law becomes:

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

Aerosol cans carry clear warnings against incineration because of the high pressures that can develop upon heating. Suppose that a can contains a residual amount of gas at a pressure of 760 mmHg and a temperature of 30 ^{o}C.

What would the pressure be if the can were heated to 1155 ^{o}C?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Chemistry Gas Laws concept. If you need more Chemistry Gas Laws practice, you can also practice Chemistry Gas Laws practice problems.