A mixture initially contains A, B, and C in the following concentrations: [A] =

Question

A mixture initially contains A, B, and C in the following concentrations: [A] = 0.700 M , [B] = 0.600 M, and [C] = 0.400 M . The following reaction occurs and equilibrium is established:

A+2BC

At equilibrium, [A] = 0.600 M and [C] = 0.500 M . Calculate the value of the equilibrium constant, Kc.

A mixture initially contains A, B, and C in the following concentrations: LA] -0.700 M,B]- 0.600 M and Cl 0.400 M The following reaction occurs and equilibrium is established: A 2B At equilibrium, LA] 0.600 M and Cl 0.500 M. Calculate the value of the equilibrium constant, Kc Express your answer numerically. Kc

Explanation / Answer

First, write the balanced chemical equation with an ICE table.

A + 2B C

I/mol·L-1: 0.700; 0.600; 0.400
C/mol·L-1: -x; -2x; +x
E/mol·L-1: 0.700- x; 0.600-2x; 0.400 +x

At equilibrium, [A] mol/L = 0.600mol/L = (0.700 - x) mol/L

So x = 0.700 – 0.600 = 0.100

[B] = (0.600 - 2x) mol/L = (0.600– 2×0.100) mol/L =0.400 mol/L

[C] = (0.400 +x) mol/L = (0.400 + 0.100) mol/L = 0.500 mol/L

Now, Kc = [C] /[A][B]2

=0.500 /0.600 x (0.400)2

=0.500 /0.096

=5.208 =5.21

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