Calculate the entropy change (J/mol K) of the given reaction. The molar entropies (J/mol K) are given in brackets after each substance :2PbS(s)[91.2]+3O2(g)[205.1]⟶2PbO(s)[66.5]+2SO2(g)[248.2]

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Calculate the entropy change $(J / mol K)$ of the given reaction. The molar entropies $(J / mol K)$ are given in brackets after each substance :

$2 PbS (s) [91 .2] + 3 O_{2} (g) [205 .1] ⟶ 2 PbO (s) [66.5] + 2 {SO}_{2} (g) [248.2]$

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+72.5

-149.2

-113.5

-168.3

answer is B.

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Detailed Solution

Change in entropy is the difference of Sum of entropy of the product and the Sum of entropy of reactant. Thus,

$ΔS = {(2 \times 66.5) + (2 \times 248.2)} - {(2 \times 91.2) + (3 \times 205.1)}$

$ΔS = - 168.3 \frac{J}{mol K}$

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