Which is the correct equilibrium constant expression FeO(s) + H_2(g) Fe(s) + H_2

Question

Which is the correct equilibrium constant expression FeO(s) + H_2(g) Fe(s) + H_2O(g) a) K_c = [Fe][H_2O]/[e_2O_3] b) K_c = [H_2O]/[H_2] c) K_c = [Fe_2O_3][H_2]/[Fe][H_2O] d) K_c = [Fe][H_2O]/[Fe_2O_3][H_2] e)K_c = [H_2]/[H_2O] What is the equilibrium constant, K_c, for an equilibrium mixture for the reac 2BrCl_3(g) Br_2(g) + 3Cl_2(g) was found to contain 2.0 mol BrCl_3, 3.0 mol mol Cl_2 in a 4.0 L vessel. a) 5.9 b) 108 c) 1.2 d) 18 e) 432 Phosgene, COCl_2, a poisonous gas, decomposes according to the equation COCl_2(g) CO(g) + Cl_2(g). Calculate K_p for this reaction if K_c = 0.09 R = 0.0821 L middot atm/(K mol)) 0.13 0.78 6.1 0.083

Explanation / Answer

1. Correct equilibrium constant expression would be,

b) Kc = [H2O]/[H2]

2. Given,

2BrCl3 <==> Br2 + 3Cl2

with,

molarity = moles/L of solution

thus,

[BrCl3] = 2 mol/4 L = 0.5 M

[Cl2] = 3.0 mol/4 L = 0.75 M

[Br2] = 1 mol/4 L = 0.25 M

we get,

Kc = [Br2][Cl2]^3/[BrCl3]^2

      = (0.25)(0.75)^3/(0.5)^2

      = 0.422

Answer : e) 0.432

[note: the e) value is incorrectly written, it should be 0.432 and not 432]

3. for the given reaction,

Kp = Kc(RT)^dn

with,

dn = 2 - 1 = 1

R = gas constant

T = 298 K

Kc = 0.092

we get,

Kp = 0.092(0.0821 x 298)^1

      = 2.2

answer : e)

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