Calculate ΔG° for each of the following reactions from the equilibrium constant at the temperature given.(a) N2(g) + O2(g) ⟶ 2NO(g) T = 2000 °C K p = 4.1 × 10−4(b) H2(g) + I2(g) ⟶ 2HI(g) T = 400 °C K p = 50.0(c) CO2(g) + H2(g) ⟶ CO(g) + H2 O(g) T = 980 °C K p = 1.67(d) CaCO3(s) ⟶ CaO(s) + CO2(g) T = 900 °C K p = 1.04(e) HF(aq) + H2 O(l) ⟶ H3 O+(aq) + F−(aq) T = 25 °C K p = 7.2 × 10−4(f) AgBr(s) ⟶ Ag+(aq) + Br−(aq) T = 25 °C K p = 3.3 × 10−13

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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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Calculate ΔG° for each of the following reactions from the equilibrium constant at the temperature given.
(a) N₂(g) + O₂(g) ⟶ 2NO(g) T = 2000 °C K _p = 4.1 × 10⁻⁴
(b) H₂(g) + I₂(g) ⟶ 2HI(g) T = 400 °C K _p = 50.0
(c) CO₂(g) + H₂(g) ⟶ CO(g) + H₂ O(g) T = 980 °C K _p = 1.67
(d) CaCO₃(s) ⟶ CaO(s) + CO₂(g) T = 900 °C K _p = 1.04
(e) HF(aq) + H₂ O(l) ⟶ H₃ O⁺(aq) + F⁻(aq) T = 25 °C K _p = 7.2 × 10⁻⁴
(f) AgBr(s) ⟶ Ag⁺(aq) + Br⁻(aq) T = 25 °C K _p = 3.3 × 10⁻¹³

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