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(a) Calculate K at 298 K for the following reaction: NO(g) + O₂(g) = NO₂(g) 2 K= 1.741 Part 2 out of 2 (H): NO(g) 86.60 NO₂(g) 51 0₂(8) 0 AG⁰ = AG x 10 (b) Use the equilibrium constant to calculate AGº (in kJ) at 298 K for the following reaction: 2HCl(g) → H₂(g) + Cl₂(g) K= 3.89 × 10-34 at 298 K mol x 10 kJ

(a) Calculate K at 298 K for the following reaction: NO(g) + O₂(g) = NO₂(g) 2 K= 1.741 Part 2 out of 2 (H): NO(g) 86.60 NO₂(g) 51 0₂(8) 0 AG⁰ = AG x 10 (b) Use the equilibrium constant to calculate AGº (in kJ) at 298 K for the following reaction: 2HCl(g) → H₂(g) + Cl₂(g) K= 3.89 × 10-34 at 298 K mol x 10 kJ

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 106CP
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(a) Calculate K at 298 K for the following reaction: 1 NO(g) + O₂(g) ⇒ NO₂(g) K = 1.741 NO(g) 86.60 NO₂(g) 51 O₂(g) 0 Part 2 out of 2 AG () f mol AG⁰ = x 10 (b) Use the equilibrium constant to calculate AGº (in kJ) at 298 K for the following reaction: 2HCl(g) → H₂(g) + Cl₂(g) K = 3.89 × 10-34 at 298 K x 10 kJ
Transcribed Image Text:(a) Calculate K at 298 K for the following reaction: 1 NO(g) + O₂(g) ⇒ NO₂(g) K = 1.741 NO(g) 86.60 NO₂(g) 51 O₂(g) 0 Part 2 out of 2 AG () f mol AG⁰ = x 10 (b) Use the equilibrium constant to calculate AGº (in kJ) at 298 K for the following reaction: 2HCl(g) → H₂(g) + Cl₂(g) K = 3.89 × 10-34 at 298 K x 10 kJ
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