(iii) At a temperature of 300 °C the free Gibbs energy is 25.0 kJ mol-¹. Calculate the equilibrium constant, K, at this temperature. AFG = -RTINK. K= P 4 2 9 8 7 A 0 8 2 0 (iv) Comment on the equilibrium using the value of K you have calculated. (2) (no units)

(iii) At a temperature of 300 °C the free Gibbs energy is 25.0 kJ mol-¹. Calculate the equilibrium constant, K, at this temperature. AFG = -RTINK. K= P 4 2 9 8 7 A 0 8 2 0 (iv) Comment on the equilibrium using the value of K you have calculated. (2) (no units)

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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Question

(iii) At a temperature of 300 °C the free Gibbs energy is 25.0 kJ mol-¹.
Calculate the equilibrium constant, K, at this temperature.
AFG = -RTINK.
K=
P 4 2 9 8 7 A 0 8 2 0
(iv) Comment on the equilibrium using the value of K you have calculated.
(2)
(no units)

lodine pentoxide, I₂O5, is a white crystalline solid. It is formed by heating HIO, to
about 200 °C in a stream of dry air. The reaction is shown below.
2HIO₂ (s) 1₂0,(s) + H₂O(g)

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