Problem: A mixture initially contains A, B, and C in the following concentrations: [A] = 0.350 M, [B] = 1.40 M, and [C] = 0.700 M. The following reaction occurs and equilibrium is established: A + 2B ⇌ C At equilibrium, [A] = 0.170 M and [C] = 0.880 M. Calculate the value of the equilibrium constant, Kc. Express your answer numerically.

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FREE Expert Solution

We are being asked to calculate the equilibrium constant, Kc for the given equilibrium reaction:

A + 2B  C


When dealing with equilibrium and Kc:

Kc → equilibrium units are in molarity 
Kc is an equilibrium expression:

Kc=productsreactants

only aqueous and gaseous species are included in the equilibrium expression
▪ the coefficient of each compound in the reaction equation will be the exponent of the concentrations in the equilibrium expression


Given:    

98% (70 ratings)
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Problem Details

A mixture initially contains A, B, and C in the following concentrations: [A] = 0.350 M, [B] = 1.40 M, and [C] = 0.700 M. The following reaction occurs and equilibrium is established: 

A + 2B ⇌ C 

At equilibrium, [A] = 0.170 M and [C] = 0.880 M. Calculate the value of the equilibrium constant, Kc

Express your answer numerically.


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