# Given constant volume, what pressure would 50*atm of gas at 0 ""^@C, develop at a temperature of 300 ""^@C?

Gay Lusaac's law holds that at constant volume, $\left(\frac{{P}_{1}}{T} _ 1 = \frac{{P}_{2}}{T} _ 2\right)$ (i.e. pressure is proportional to temperature at constant volume).
So, ${P}_{2}$ $=$ $\frac{{P}_{1} {T}_{2}}{T} _ 1$ $=$ $\frac{50.0 \cdot a t m \times 273 K}{573 K}$ $=$
?? atmospheres
This is reasonable on the basis that we would expect a given quantity of gas to exert less pressure at lower temperature. Note that I converted the temperature to the Kelvin scale in order to avoid multiplying by $0$.