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Question

1.0 mol of PCl3(g) and 2.0 mol of Cl2(g) were placed in a 3 L flask and heated to 400 K. When equilibrium was established, only 0.70 mol of PCl3(g) remained. What is the value of equilibrium constant for the reaction:
PCl3(g)+Cl2(g)PCl5(g) at 400 K?

A
0.25
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B
1.31
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C
0.76
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D
2.6
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Solution

The correct option is C 0.76
The following table lists the number of moles of different species.
PCl3 Cl2 PCl5
Initial 1 2 0
change -x -x x
Equilibrium 1 - x 2 - x x
But at equilibrium, [PCl3]=0.7=1xx=0.3
Thus, the number of moles of PCl3,Cl2 and PCl5 are 0.7, 1.7 and 0.3 respectively.
The molar concentrations of PCl3,Cl2 and PCl5 are 0.73M,1.73M and 0.33M respectively.
So, According to definition of equilibrium constant.
So, Kc=(0.3)(3)(1.7)(0.7)=0.76

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