Question

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?

Answer 1

`P_2=0.360atm`

Explanation:

Assuming that Hydrogen is behaving ideally, therefore, we can use the ideal gas law:`PV=nRT`

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

`P/T=k` where `k=(nR)/V` is a constant value that does not change during the process.

Thus, `(P_1)/(T_1)=(P_2)/(T_2)` This is called Gay-Lussac law.

`=>P_2=(P_1)/(T_1)xxT_2`

`=>P_2=(0.329atm)/(320cancel(K))xx350cancel(K)=0.360atm`