Question 9 (1 point)

For the following equilibrium system at 100^oC, calculate Gibb's free energy (G) and determine the approximate composition of the equilibrium system.

2 NO(g) + O₂(g) 2 NO₂(g) H = -120 kJ/mol; S = - 0.150 kJ/(K.mol)

Question 9 options:

	-64 kJ/mol; 50-90% reactants
	-64 kJ/mol; 50-90% products
	- 105 kJ/mol; 50-90% products
	- 105 kJ/mol; > 90% reactants
	- 105 kJ/mol; 50-90% reactants

Question 10 (1 point)

Consider the equilibrium for the decomposition of nitrosyl chloride:

2 NOCl (g) + energy <--> 2 NO (g) + Cl₂ (g)

What set of conditions will result in the greatest shift in the forward direction?

Question 10 options:

	decrease volume, decrease temperature
	increase volume, increase temperature
	increase pressure by adding a noble gas, decrease temperature
	increase volume, decrease temperature
	decrease volume, increase temperature

Question 11 (1 point)

Consider the Haber-Bosch process:

N_2(g) + 3H_2(g) <--> 2NH_3(g) K = 6.0 x 10^-2 @ 500^oC

The process was carried out at 500^oC, and the concentrations of each gas are analyzed.

Given that the concentration of ammonia is 2.0 x 10^-4 mol/L, nitrogen gas is 1.5 x10^-5 mol/L and hydrogen gas is 3.5 x 10^-5 mol/L, what does the Q value indicate?

Question 11 options:

	The system is at equilibrium.
	The system is not at equilibrium; shift to the products
	The system is not at equilibrium; shift to the reactants
	The reaction rate is speeding up