Question
In: Chemistry
A mixture initially contains A, B, and C in the following concentrations: [A] = 0.700M ,...
A mixture initially contains A, B, and C in the following concentrations: [A] = 0.700M , [B] = 0.850M , and [C] = 0.400M . The following reaction occurs and equilibrium is established:
A+2B?C
At equilibrium, [A] = 0.560M and [C] = 0.540M . Calculate the value of the equilibrium constant, Kc.
Solutions
Expert Solution
Kc = [C] / ([A] * [B]2])
As you see, the amount of moles of C formed is 0.140, so, in the following reaction x = 0.140:
A + 2B ---> C
initial 0.7 0.85 0.4
change -x -2x +x
end (eq) 0.7-x 0.85-2x 0.4+x
final [B] = 0.85 - (2*0.140) = 0.57
Kc = (0.540) / (0.560) * (0.570)2 = 0.540 / 0.182 =
2.97
queen_honey_blossom answered 1 hour agoRelated Solutions
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