35. What is the consequence of heating the following equilibrium system to a hig

Question

35. What is the consequence of heating the following equilibrium system to a higher temperature?

2NH3 (g) N2 (g) + 3 H2 (g)            H° = +92.4 kJ/mol

A. The concentration of N2 will decrease, and the equilibrium constant will decrease.

B. The concentration of NH3 will decrease, and the equilibrium constant will decrease.

C. The concentration of NH3 will increase and the equilibrium constant will increase.

D. The concentration of N2 will increase, and the equilibrium constant will increase.

E. The concentration of N2 will increase and the equilibrium constant will decrease.

36. Consider the following reactions at equilibrium and determine which of the indicated changes will cause the reaction to proceed to the left. I. 2H2Og 2H20g +O2 (g) remove water) II. H2 (g) +I2 (g) g) remove HI) III. CaCO3 (s) CaOCs) +CO2 (g) rease pressure) V. Baos) SO3 (g) BasO4 (s) (increase volume A. I and III B. II and III C. III and IV D. I and V E. II and V

Explanation / Answer

Q.No-35

Given 2NH3 (g) N2 (g) + 3 H2 (g)            H° = +92.4 kJ/mol

When temperature increases during above reaction , more N2 gas will produce hence concentration of N2 will increase.

Equilibrium constant, Keq = [N2][H2]3 / [NH3]2

According to above expression, Keq is directly propotional to [N2], so equilibrium constant will increase.

Correct answer is (D)

Q.N0-36

Correct answer is (B)

According to Lechateriels princple, these two reactions ( II & III ) will proceed to left. For more information just go through The Chateriels Principle.

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