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  • Calculate the entropy change in surroundings when 1.00 mol of H2O(l) is formed under standard conditions. delta f H = –286 kJ mol–1.

6.22   Calculate the entropy change in surroundings when 1.00 mol ofH_2 O (l) is formed under standard conditions. \Delta _f H ^ \ominus = -286 KJ mol ^ { -1} 

Answers (1)

best_answer

-286 kJ/mol heat is evolved when 1 mol of the water molecule is formed. It means the same amount of energy is absorbed by the surrounding also.

q_{surr}= +286kJ/mol
We know that,
Entropy changes for the surrounding is  = q(surr)/ temp.
                                                                = 286000/ 298

                                                                = 959.73 J/mol/K

Posted by

manish

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