Enthalpy change for freezing of $1 g$ of water at $1 \mathrm{bar}$ and $0^{\circ} \mathrm{C}$ is $334…
Enthalpy change for freezing of $1 g$ of water at $1 \mathrm{bar}$ and $0^{\circ} \mathrm{C}$ is $334 \mathrm{~J}$. Calculate the internal energy change in $J$ when $1 \mathrm{~g}$ of water is converted into ice?
205
334
0
668
Solution
When $1 \mathrm{~g}$ water is converted into ice then internal energy is equal to enthalpy change for freezing at 1 bar and $0^{\circ} \mathrm{C}$.
$$
\operatorname{lg~} \mathrm{H}_2 \mathrm{O}(\mathrm{aq}) ightleftharpoons \mathrm{H}_2 \mathrm{O} \text { (ice) }
$$
Enthalpy change for freezing of $1 \mathrm{~g}$ of water at 1 bar and $0^{\circ} \mathrm{C}$ temperature is $334 \mathrm{~J}$.
Hence, internal energy equal to $334 \mathrm{~J}$.
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