JEE Chemistry 2024 Question with Solution

Given: Standard enthalpy of vaporization of $\text{CCl}_4$ is $30.5 \, \text{kJ mol}^{-1}$ and mass is $284 \, \text{g}$.

Find: Heat required for vaporization of the given mass of $\text{CCl}_4$.

First, calculate the molar mass of $\text{CCl}_4$:

Now calculate the number of moles:

Use the enthalpy of vaporization relation:

Therefore, the heat required is approximately $56 \, \text{kJ}$. The correct option is A.

Given: $\Delta H_{\text{vap}}^\circ$ for $\text{CCl}_4$ is $30.5 \, \text{kJ/mol}$.

Find: Heat needed for $284 \, \text{g}$ of $\text{CCl}_4$.

For $1$ mole of $\text{CCl}_4$, heat required is $30.5 \, \text{kJ}$.

Molar mass of $\text{CCl}_4$ is:

So, moles in $284 \, \text{g}$ are:

Hence, heat required is:

Thus, the answer rounds to $56 \, \text{kJ}$. The correct option is A.