Question

At ${47}^0$C and $16$ atm, the molar volume of $N{H}_3$ gas is about $10\%$ less than the molar volume of an ideal gas. This is due to:

• A. $N{H}_3$ decomposes to $N_2$ and $H_2$ at ${47}^0$C
• B. the force of attraction between molecules is significant at this temperature and pressure
• C. the volume occupied by $N{H}_3$ molecules themselves is a significant fraction of the volume of the container at this temperature and pressure
• D. at $16$ atm, $N{H}_3$ molecules no longer move randomly

Answer 1

The correct option is B the force of attraction between molecules is significant at this temperature and pressure

Real gases unlike gases, have atoms which occupy volume and interact with one other.

$\Rightarrow$ At ${47}^{0}C$ or $320K$, and $16$ atm, the intermolecular dorces of attraction for ${NH}_3$ become significant.

Option - B is correct.