Question

The molar enthalpy change for $H_{2}O\left(1\right)\rightleftharpoons H2O\left(g\right)$ at $373$K and $1$ atm is $41$kJ/mol. Assuming ideal behavior, the internal energy change for vaporization of $1$ mol of water at $373$K and $1$ atm in kJ $mo{l}^{-1}$ is $?$

• A. $30.2$
• B. $41.0$
• C. $48.1$
• D. $37.9$

Answer 1

The correct option is D $37.9$

$W=-nRT=1(8.314\times 373)\times {10}^{-3}=-3.10KJ$

$q=41KJ$

$\Delta U=37.9KJ$