Consider the reaction
2A+3B-> C +4D
You mix 500ml of 1.0M A, and 500ml of 1.4 M B. At equilibrium, you detect C to have a concentration of 0.218M. What is the equilibrium constant for this reaction?
Given reaction 2A+3B-> C +4D
but the term "D" is not involved in the determination of equilibrium constant as its concentration is not mentioned,
A concentration will be = 500 mL x 10-3 L x 1.0 m = 0.5M
B concentration will be = 500 mL x 10-3 L x 1.4 m = 0.7M
when we mixed these two total volume becomes 1000 mL = 1L, hence C concentration remains unchanged
as molarity (M) = moles / liter
Keq = [C] / [2A]2 [3B]3 = 0.218 / [2 x 0.5]2 [ 3 x 0.7]3 = 0.02354
Keq = 0.02354
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