# A sample of hydrogen at 47°C exerts a pressure of .329 atm. The gas is heated to 77°C at constant volume. What will its new pressure be?

Nov 28, 2015

${P}_{2} = 0.360 a t m$

#### Explanation:

Assuming that Hydrogen is behaving ideally, therefore, we can use the ideal gas law:$P V = n R T$

Since the gas is being heated only and the volume is not changing, therefore, n and V are constant and therefore we can say:

$\frac{P}{T} = k$ where $k = \frac{n R}{V}$ is a constant value that does not change during the process.

Thus, $\frac{{P}_{1}}{{T}_{1}} = \frac{{P}_{2}}{{T}_{2}}$ This is called Gay-Lussac law.

$\implies {P}_{2} = \frac{{P}_{1}}{{T}_{1}} \times {T}_{2}$

$\implies {P}_{2} = \frac{0.329 a t m}{320 \cancel{K}} \times 350 \cancel{K} = 0.360 a t m$