Consider the following system at equilibrium where H° = -111 kJ/mol, and Kc = 0.159, at 723 K. N2(g) + 3H2(g) 2NH3(g) If the TEMPERATURE on the equilibrium system is suddenly decreased:The value of Kcfill in the blank 1A. increases. B. decreases. C. remains the same. The value of Qfill in the blank 2A. is greater than Kc. B. is equal to Kc. C. is less than Kc. The reaction must:fill in the blank 3A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The concentration of H2 will:fill in the blank 4A. increase. B. decrease. C. remain the same.

Given that ∆H° = -111 kJ/mol Hence the reaction is exothermic in nature. This means the forward…

Answered: Consider the following system at…

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...

See similar textbooks

Related questions

Question

Consider the following system at equilibrium where H° = -111 kJ/mol, and K_c = 0.159, at 723 K. N₂(g) + 3H₂(g) 2NH₃(g) If the TEMPERATURE on the equilibrium system is suddenly decreased:

The value of K_c	fill in the blank 1	A. increases.
		B. decreases.
		C. remains the same.

The value of Q	fill in the blank 2	A. is greater than K_c.
		B. is equal to K_c.
		C. is less than K_c.

The reaction must:	fill in the blank 3	A. run in the forward direction to reestablish equilibrium.
		B. run in the reverse direction to reestablish equilibrium.
		C. remain the same. It is already at equilibrium.