Calculate the entropy change in surroundings when 1.00 mol of H₂O_{( l )} is formed under standard conditions. Δ_fH^θ = 286 kJ mol¹.

Formation of H₂O(l) is an exothermic process.So, ΔH= -286 kJ/mol

Therefore, heat is transferred to the surroundings.

Thus, q_surr = +286 kJ/mol

Now, ΔS = q/t

 = (286 x 1000) / 298  

 = 959 JK^-1mol^-1