A.) The equilibrium constant for the reaction A(g) ⇌B(g) is 10² . A reaction mixture initiallycontains [A] = 18.6 M and [B] = 0.0 M. Which statement is true atequilibrium?

	The reaction mixture contains [A] = 18.4 M and [B] = 0.2M.
	The reaction mixture contains [A] = 0.2 M and [B] = 18.4M.
	The reaction mixture contains [A] = 1.0 M and [B] = 17.6M.
	The reaction mixture contains [A] = 9.30 M and [B] = 9.30M.

B.) Determine the value of K_c for the followingreaction if the equilibrium concentrations are as follows:[H₂]_eq = 0.14 M, [F₂]_eq = 0.39 M, [HF]_eq = 1.6M.

H₂(g) + F ₂(g) ↔ 2 HF(g)

	3.4 × 10-2
	29
	8.7 × 10-2
	47
	2.1 × 10-2

C.) The equilibrium constant isequal to 5.00 at 1300 K for the reaction:

2 SO₂(g) + O₂(g) ↔ 2SO₃(g).

If initial concentrations are [SO₂] = 3.60 M,[O₂] = 0.45 M, and [SO₃] = 5.40 M, the systemis

	not at equilibrium and will shift to the left to achieve anequilibrium state.
	not at equilibrium and will remain in an unequilibratedstate.
	at equilibrium.
	not at equilibrium and will shift to the right to achieve anequilibrium state.

D.) The equilibriumconstant, K_p, equals 3.40 for theisomerization reaction:

cis-2-butene ↔ trans-2-butene.
If a flask initially contains 0.250 atm of cis-2-buteneand 0.165 atm of trans-2-butene, what is the equilibriumpressure of each gas?

	P(cis-2-butene) = 0.0458 atm andP(trans-2-butene) = 0.156 atm
	P(cis-2-butene) = 0.0735 atm andP(trans-2-butene) = 0.250 atm
	P(cis-2-butene) = 0.0485 atm andP(trans-2-butene) = 0.165 atm
	P(cis-2-butene) = 0.0943 atm andP(trans-2-butene) = 0.321 atm

E.) Consider the reactionSO₂(g) +NO₂(g) ↔ NO(g) +SO₃(g) at 460°C.What is the equilibrium concentration of the SO₃if the initial concentrations are[SO₂] =[NO₂] = 3.00 x10^-3 M and [NO] =[SO₃] = 4.00 x10^-2 M? The valueof the equilibrium constant for the reaction is 85.0 at460°C.

	7.72 x 10-3 M
	8.15 x 10-2 M
	4.20 x 10-3 M
	1.80 x 10-3 M
	4.56 x 10-2 M
	3.88 x 10-2 M