35
Question
If the initial concentrations in a particular mixture of reactants and products are [PCl5]=0.5M,[PCl3]=0.15M, and [Cl2]=0.6M, the direction in which the reaction proceed to reach equilibrium is:
If the initial concentrations in a particular mixture of reactants and products are [PCl5]=0.5M,[PCl3]=0.15M, and [Cl2]=0.6M, the direction in which the reaction proceed to reach equilibrium is:
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Solution
The correct option is B to the right, [PCl5]=0.365M;[PCl3]=0.285M;[Cl2]=0.735M
Initially, 1 mole of PCl5 is present.
78.5 % of it dissociates to reach equilibrium. Hence,
1×78100=0.785 of it will dissociate to reach equilibrium.
The number of moles of PCl5,PCl3 and Cl2 present at equilibrium are 0.215, 0.785 and 0.785 respectively.
The equilibrium constant is K=[PCl3][Cl2][PCl5]
K=0.78550.78550.2155=0.573
The reaction quotient is Q=[PCl3][Cl2][PCl5]
Q=0.15×0.60.5=0.18
Since, the value of the reaction quotient is smaller than the value of the equilibrium constant, the reaction will shift in the forward direction, i.e to the right.
The initial concentrations in a particular mixture of reactants and products are [PCl5]=0.5M,[PCl3]=0.15M, and [Cl2]=0.6M,
The equilibrium concentrations in a particular mixture of reactants and products are
[PCl5]=0.5−xM,[PCl3]=0.15+xM, and [Cl2]=0.6+xM
The equilibrium constant expression is K=[PCl3][Cl2][PCl5]
K=(0.15+x)(0.6+x)0.5−x=0.573
0.09+0.75x+x2=0.2865−0.573x
x2+1.323x−0.1965
x=0.1348 or x=−1.46
Negative value is discarded as concentration cannot have negative value.
The equilibrium concentrations in a particular mixture of reactants and products are [PCl5]=0.5−0.1348=0.365M,[PCl3]=0.15+0.1348=0.285M, and [Cl2]=0.6+0.1348=0.735M
Initially, 1 mole of PCl5 is present.
78.5 % of it dissociates to reach equilibrium. Hence,
1×78100=0.785 of it will dissociate to reach equilibrium.
The number of moles of PCl5,PCl3 and Cl2 present at equilibrium are 0.215, 0.785 and 0.785 respectively.
The equilibrium constant is K=[PCl3][Cl2][PCl5]
K=0.78550.78550.2155=0.573
The reaction quotient is Q=[PCl3][Cl2][PCl5]
Q=0.15×0.60.5=0.18
Since, the value of the reaction quotient is smaller than the value of the equilibrium constant, the reaction will shift in the forward direction, i.e to the right.
The initial concentrations in a particular mixture of reactants and products are [PCl5]=0.5M,[PCl3]=0.15M, and [Cl2]=0.6M,
The equilibrium concentrations in a particular mixture of reactants and products are
[PCl5]=0.5−xM,[PCl3]=0.15+xM, and [Cl2]=0.6+xM
The equilibrium constant expression is K=[PCl3][Cl2][PCl5]
K=(0.15+x)(0.6+x)0.5−x=0.573
0.09+0.75x+x2=0.2865−0.573x
x2+1.323x−0.1965
x=0.1348 or x=−1.46
Negative value is discarded as concentration cannot have negative value.
The equilibrium concentrations in a particular mixture of reactants and products are [PCl5]=0.5−0.1348=0.365M,[PCl3]=0.15+0.1348=0.285M, and [Cl2]=0.6+0.1348=0.735M
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