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Calculate the entropy change in surround...

Calculate the entropy change in surroundings when `1.00` mol of `H_(2)O(l)` is formed under standard conditions, `Delta_(r )H^(Θ) = -286 kJ mol^(-1)`.

Text Solution

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Enthalpy change for the formation of 1 mole of `H_(2)O` (l),.
`H_(2)(g) + 1/2O_(2)(g) to H_(2)O(l), DeltaH_(f)H^(@) = -286 kJ mol^(-1)`
Energy related in the above reaction, is absorbed by the surroundings.
It means `q_("surr") = +286 kJ mol^(-1)`
`DeltaS = (q_("sur"))/(T) = (+286 kJ mol^(-1))/(298 K) = 09597 kJK^(-1) mol^(-1) = 959.7 JK^(-1) mol^(-1)`
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