Question

Molar enthalpy change for melting of ice is $6\, kJ / mol$. Then the internal energy change (in $k J / mol$ ) when $1$ mole of water is converted into ice at $1$ atm at $0^{\circ} C$ is Empty QImg

• A. RT/1000
• B. 6
• C. 6-(RT/1000)
• D. 6+(RT/1000)

Answer 1

Answer: (B)

6

Answer 2

Given, $\Delta H=6\, kJ / mol$ $\Delta U=?$ $H_{2} O(l) Ice(s)$ $\because \Delta H=\Delta U+\Delta n_{g} R T$ Here, $\Delta n_{g}=0$ $\therefore \Delta H=\Delta U$ $\Rightarrow \Delta U=6\, kJ / mol$