Analyzing reaction at equilibrium

Question

Assignment:

Q1. K_c for the reaction below at 25°C is 4.8 x 10^-6. Calculate the equilibrium concentration (mol/L) of Cl₂(g) if the initial concentration of ICl(g) is 1.33 mol/L. There is no I2 or Cl2 initially present.

2ICl(g) <-> I₂(g) + Cl₂(g)

a. 6.4 x 10-6
b. 343
c. 3.2 x 10-6
d. 2.9 x 10-3
e. 5.8 x 10-3

Q2. Consider the following reaction at equilibrium:

2NH₃(g) <-> N₂(g) + 3H₂(g) ΔH° = +92.4 kJ

Adding N₂(g) to the system at equilibrium will __________.

a. decrease the concentration of H₂(g) at equilibrium
b. remove all of the H₂(g)
c. cause the reaction to shift to the right
d. increase the value of the equilibrium constant
e. decrease the concentration of NH₃(g) at equilibrium

Q4. Consider the following reaction at equilibrium:

2CO₂(g) <-> 2CO(g) + O₂(g) ΔH° = 514 kJ

Increasing the temperature will ________.

a. decrease the concentration of CO₂(g)
b. shift the reaction to the right
c. increase the concentration of CO
d. increase the concentration of O₂(g)
e. decrease the value of the equilibrium constant

Q5. The effect of a catalyst on a chemical reaction is to
_______________.

a. accelerate the forward reaction only
b. lower the energy of the transition state
c. make reactions more exothermic
d. increase the entropy change associated with a reaction
e. react with product, effectively removing it and shifting the
equilibrium to the right

Q6. Consider the equilibrium at 25°C:
1A(g) + 2B(g) <-> 3C(g) + D(L) Kc = 3.25 x 10^-2
What is the value of Kp?

a. 19.453700
b. 80.521090
c. 0.136915
d. 0.000156
e. 0.032500

Q7. Consider the equilibrium at 25°C:
2A(g) + 2B(g)<-> 1C(g) + D(L) Kp = 2.65 x 10^-4

What is the value of Kc?

a. 4030182.628
b. 3.881
c. 1586.224730
d. 0.002291
e. 2379.556