Problem: Consider the following reaction: 2 NO(g) + O2(g) → 2 NO2(g)Estimate ΔG˚ for this reaction at each of the following temperatures and predict whether or not the reaction will be spontaneous. (Assume that ΔH˚ and ΔS˚ do not change too much within the give temperature range.)851 K

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FREE Expert Solution

Step 1

H°rxn = H°product -H°reactantH°rxn =[2 mol NO2(33.2 kJ1 mol NO2)]                 - [2 mol NO(91.3 kJ1 mol NO) + 0]H°rxn =66.4 kJ - 182.6 kJ

ΔH°rxn = -116.2 kJ


Step 2

S°rxn = S°product -S°reactantS°rxn =[2 mol NO2(240.1 J1 mol NO2·K)]                - [2 mol NO(210.8 J1 mol NO·K)+1 mol O2(205.2 J1 mol O2·K)]S°rxn = 480.2 JK - 626.8 JKS°rxn =-146.6 JK×1 kJ103 J

ΔS°rxn = - 0.1466 kJ/K


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Problem Details

Consider the following reaction: 2 NO(g) + O2(g) → 2 NO2(g)

Estimate ΔG˚ for this reaction at each of the following temperatures and predict whether or not the reaction will be spontaneous. (Assume that ΔH˚ and ΔS˚ do not change too much within the give temperature range.)

851 K