Answer:
K = 0.0396
Explanation:
Based on the reaction:
A + 2B ⇄ 3C + 2D
Where equilibrium constant, K, is:
K = [C]³[D]² / [A] [B]²
The initial concentrations of A and B are:
[A]₀ = 0.050M * (45.0mL / 70.0mL) = 0.0321M
[B]₀ = 0.100M * (25.0mL / 70.0mL) = 0.0357M
As [C] = 0.0410M, the molar concentration of D is:
0.0410M * (2mol D / 3mol C) = 0.0273M = [D]
And the concentration of A and B that reacted was:
0.0410M * (2mol B / 3mol C) = 0.0273M B
0.0410M * (1mol A / 3mol C) = 0.0137M A
Equilibrium concentration B and A:
0.0357M - 0.0273M = 0.0084M = [B]
0.0321M - 0.0137M = 0.0184M = [A]
And K is:
K = [0.0410M]³[0.0273M]² / [0.0184M] [0.0084M]²
K = 0.0396
