Question

Part A

Dinitrogen tetroxide decomposes to form nitrogen dioxide according to the following reaction:

N2O4(g)⇌2NO2(g), Kp=6.7N2O4(g)⇌2NO2(g), Kp=6.7 at 298K298K

A reaction vessel contains 0.45 atmatm of N2O4N2O4 and 2.0 atm NO2atm NO2.

Which statement is true of the reaction system?

A) The reaction system is at equilibrium.

B)The reaction system proceeds to the left (forming more reactant).

C)The reaction system proceeds to the right (forming more product).

D)It is impossible to determine the future progress of the reaction based on the information given.

B Consider the reaction between bromine and chlorine gases to form bromochloride:

Br2(g)+Cl2(g)⇌2BrCl(g), Kc=1.11×10−4 at 150K

A reaction vessel contains 0.20M Br2, 0.35MCl2, and 3.0×10−3M BrCl. Calculate the reaction quotient, Q, and determine in which direction the reaction proceeds to reach equilibrium.

A)1.1×10–41.1×10–4, the reaction system is at equilibrium

B)4.3×10–24.3×10–2, the reaction system proceeds to the left

C)1.3×10–41.3×10–4, the reaction system proceeds to the right

D)1.3×10−41.3×10−4, the reaction system proceeds to the left

Answer 1