Question

Question 1:

The reaction 2CH4(g)⇌C2H2(g)+3H2(g) has an equilibrium constant of K = 0.154. If 6.25 mol of CH4, 4.45 mol of C2H2, and 11.55 mol of H2 are added to a reaction vessel with a volume of 6.00 L , what net reaction will occur- answer a, b or c?

a) The reaction will proceed to the left to establish equilibrium.

b) The reaction will proceed to the right to establish equilibrium.

c) No further reaction will occur because the reaction is at equilibrium.

Question 2:

Nitrogen dioxide dimerizes according to the following reaction: 2NO2(g)⇌N2O4(g)

Kp=6.7 at 298K. A 2.25-L container contains 0.055 mol of NO2and 0.082 mol of N2O4 at 298K. Is the reaction at equilibrium? If not, in what direction will the reaction proceed- answer a, b, or c?

	a) The reaction is at equilibrium.
b)	The reaction is not at equilibrium and will shift to the left.
	c) The reaction is not at equilibrium and will shift to the right.

Question 3:

The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D]/[A][B]=6.0

What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M? Express your answer to two significant figures and include the appropriate units.

Answer 1