# A sample of carbon dioxide gas at 125°C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125°C?

Jun 12, 2017

$212$ $\text{torr}$

#### Explanation:

Let's use the combined gas law:

$R i g h t a r r o w \frac{{P}_{1} {V}_{1}}{{T}_{1}} = \frac{{P}_{2} {V}_{2}}{{T}_{2}}$

In our case, the temperature of ${125}^{\circ}$ $\text{C}$ is kept constant throughout the process, so ${T}_{1} = {T}_{2}$:

$R i g h t a r r o w \frac{{P}_{1} {V}_{2}}{{T}_{1}} = \frac{{P}_{2} {V}_{2}}{{T}_{1}}$

$R i g h t a r r o w {P}_{1} {V}_{1} = {P}_{2} {V}_{2}$

Then, let's substitute the relevant values:

$R i g h t a r r o w 248$ $\text{torr} \times 275$ $\text{L} = {P}_{2} \times 321$ $\text{L}$

Rightarrow P_(2) = frac(248 " torr" times 275 " L")(321 " L")

$\therefore {P}_{2} = 212.46105919$ $\text{torr}$

Therefore, the final gas pressure will be around $212$ $\text{torr}$.