(a) Calculate K at 298 K for the following reaction:1NO(g) + O₂(g) ⇒ NO₂(g)K = 1.741NO(g) 86.60NO₂(g) 51O₂(g) 0Part 2 out of 2AG ()f molAG⁰ =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 Kx 10kJ

(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

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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