Question

# Calculate the entropy change in surroundings when 1.00 mol of H2O(l) is formed under standard conditions at 298 K. Given ΔrH0 = - 286 kJ mol−1.

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#### H2(g)+12O2(g)⟶H2O(l)ΔfH0=−286KJ/molFrom the above equation,At 298K, when 1 mole of H2O(l) is formed, 286KJ of heat is released. The same amount of heat is absorbed by the surroundings.∴qsurr.=+286KJ/mol;T=298KAs we know that,ΔSsurr.=qsurr.T∴ΔSsurr.=286298=0.96KJ/mol−KHence the entropy change in surroundings will be 0.96KJ/mol.

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