Question

Part A a mixture contains A, B, and C in the following concentrations: [A] = .550 M, [B] = 1.10 M, and [C] = .650 M. The following reaction occurs and equilibrium is established. what is Kc?

myct/itemView?assignment ProblemID=143011484&offset=next Mrs. Graves AP Chemistry Chloe & © 55: Calculating the Equilibrium Constant and the Reaction Quotient ③ 3 of 5 Review Constants Periodic Table Part A A mixture initially contains A, B, and occurs and equilibrium is established: in the following concentrations: (A) = 0.550 M B - 1.10 M, and (C] -0.650 M. The following reaction A + 2B Calculate the value of the equilibrium constant, Ke At equilibrium, (A) = 0.350 M and C -0.850 M Express your answer numerically View Available Hint(s) 0 AED O ? Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining

Answer 1

Using the ICE table

	[A]	[B]	[C]
Initial	0.550	1.10	0.650
Change	-x	-2x	+x
Final	0.550-x	1.10-2x	0.650+x

0.550 - x = 0.350, x = 0.200

[B] = 1.10 - 2(0.200) = 0.700

[A] = 0.350, [C] = 0.850

la K = [Products (Reactants] 0.850 (0.350)(0.700)2 [4][B]2

Hence the value of Kc will be equal to 4.96

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