Enthalpy change for freezing of 1 g of water | vedclass

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Question

(B) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ is given by the equation: $\Delta H = \Delta U + P\D

Vedclass · Accepted Answer

$334$

Vedclass · Answer

(B) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ is given by the equation: $\Delta H = \Delta U + P\Delta V$. At $0^{\circ} C$ and $1 \ bar$, the change in volume $(\Delta V)$ for the freezing of $1 \ g$ of water is extremely small and negligible. Therefore, $\Delta H \approx \Delta U$. Given that the enthalpy change for freezing $1 \ g$ of water is $334 \ J$, the internal energy change is also approximately $334 \ J$.

Enthalpy change for freezing of $1 \ g$ of water at $1 \ bar$ and $0^{\circ} C$ is $334 \ J$. Calculate the internal energy change in $J$ when $1 \ g$ of water is converted into ice?

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