30.4 , kJ of heat is required to melt one mol | vedclass

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Question

(A) The relationship between enthalpy change of fusion $(\Delta H_{fus})$,entropy change of fusion $(\Delta S_{fus})$,and melting point $(T_{mp})$ is

Vedclass · Accepted Answer

$1070$

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(A) The relationship between enthalpy change of fusion $(\Delta H_{fus})$,entropy change of fusion $(\Delta S_{fus})$,and melting point $(T_{mp})$ is given by the formula: $\Delta S_{fus} = \frac{\Delta H_{fus}}{T_{mp}}$.Given: $\Delta H_{fus} = 30.4 \, kJ \, mol^{-1} = 30400 \, J \, mol^{-1}$ and $\Delta S_{fus} = 28.4 \, J \, K^{-1} \, mol^{-1}$.Substituting the values into the equation: $28.4 = \frac{30400}{T_{mp}}$.Solving for $T_{mp}$: $T_{mp} = \frac{30400}{28.4} \approx 1070.42 \, K$.Rounding to the nearest integer,the melting point is $1070 \, K$.

$30.4 \, kJ$ of heat is required to melt one mole of sodium chloride and the entropy change at the melting point is $28.4 \, J \, K^{-1} \, mol^{-1}$ at $1 \, atm$. The melting point of sodium chloride is $........... \, K$ (Nearest Integer).

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