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

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


89% (332 ratings)
View Complete Written Solution
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

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gibbs Free Energy concept. You can view video lessons to learn Gibbs Free Energy. Or if you need more Gibbs Free Energy practice, you can also practice Gibbs Free Energy practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Sharma's class at VALENCIA.