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2NO(g) + O2(g) → 2NO2(g); ΔH°= –125 kJ/mol; ΔS°= –150 J/mol•K   Below a temperature of _____ K, this reaction is spontaneous.

2NO(g) + O2(g) → 2NO2(g); ΔH°= –125 kJ/mol; ΔS°= –150 J/mol•K   Below a temperature of _____ K, this reaction is spontaneous.

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter17: Chemcial Thermodynamics
Section: Chapter Questions
Problem 17.83QE: At 298 K, G = 70.52 kJ for the reaction 2NO(g) + O2(g) 2NO2(g) (a) Calculate _G at the same...
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2NO(g) + O2(g) → 2NO2(g); ΔH°= –125 kJ/mol; ΔS°= –150 J/mol•K
 
Below a temperature of _____ K, this reaction is spontaneous.

Expert Solution
Step 1

The given reaction is:

2NO (g) + O2 (g) → 2NO2 (g)

Given data,

∆H0 = -125 kJmol-1

∆So = -150 Jmol-1K-1

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