Answer:
He have higher pressure at room temperature.
Explanation:
It is given that both the gases are kept in 5 L chambers.
Therefore, volume is constant.
Also, they both are at room temperature, so temperature is also constant.
Now, number of moles of
= ![\dfrac{Given\ mass}{Molecular \ mass}=\dfrac{5}{32}=0.16\ mol.](https://tex.z-dn.net/?f=%5Cdfrac%7BGiven%5C%20mass%7D%7BMolecular%20%5C%20mass%7D%3D%5Cdfrac%7B5%7D%7B32%7D%3D0.16%5C%20mol.)
Also, number of moles of He =![\dfrac{Given\ mass}{Molecular \ mass}=\dfrac{5}{4}=1.25\ mol.](https://tex.z-dn.net/?f=%5Cdfrac%7BGiven%5C%20mass%7D%7BMolecular%20%5C%20mass%7D%3D%5Cdfrac%7B5%7D%7B4%7D%3D1.25%5C%20mol.)
Now, according to GAS LAW,
( all terms have their usual meaning).
In this case, V, R and T are constant.
So, pressure is directly proportional to n i.e number of moles.
So, moles of He is more than moles of
.
Therefore, He have higher pressure at room temperature.
Hence , this is the required solution.