The calculated value of ΔS° = -268.13 J/K
Let's think about the following equation in balance.
2 HNO3(l) + NO = 3 NO2(g) + H2O(l) (g)
The following expression can be used to determine the standard entropy change of a reaction (S°):
S° is equal to np.Sp - nr.Sr, where ni is the number of moles in reactants and products.
The usual molar entropies of the reactants and products are given by Si.
S° is equal to [2 mol S° (HNO3(l)) + 1 mol S° (NO(g))]. - [1 mol S°(H2O(l)) + 3 mol S°(NO2(g)]
[2 mol. 155.6 J/K.mol + 1 mol. 210.76 J/K] = S° .mol] - [1 mol 69.91 J/k + 3 mol 240.06 J/K.mol .mol]
ΔS° = -268.13 J/K
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