# A gas at 52°C occupies 6.8 L at a pressure of 1.5 atm. What will the pressure be at -43°C if the volume is reduced to 2.2 L?

Jun 1, 2016

The combined gas law holds that $\frac{{P}_{1} {V}_{1}}{T} _ 1$ $=$ $\frac{{P}_{2} {V}_{2}}{T} _ 2$. Thus ${P}_{2} \cong 3 \cdot a t m$.

#### Explanation:

${P}_{2} = \frac{{P}_{1} {V}_{1} {T}_{2}}{{T}_{1} {V}_{2}}$ $=$ $\frac{1.5 \cdot a t m \times 6.8 \cdot L \times 230 \cdot K}{325 \cdot K \times 2.2 \cdot L}$ $=$ ??*atm

Note that we had to convert all temperature readings to the absolute scale, as we typically do for gas problems.