For a reaction, HCl(aq)+NaOH(aq)⇌NaCl(aq)+H2O(l)GivenKc=0.5,[HCl]=3M,[NaOH]=4M,[NaCl]=6M
Find Qc and the direction in which reaction will shift.
A
Qc=0.5 ; reaction shifts in backward direction
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B
Qc=0.5 ; reaction shifts in forward direction
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C
Qc=0.5 ; reaction is at equilibrium
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D
Qc=1 ; reaction shifts in backward direction
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Solution
The correct option is CQc=0.5 ; reaction is at equilibrium Finding Qc:
Qc=[NaCl(aq)][HCl(aq)][NaOH(aq)]=63×4=0.5
Given Kc=0.5
Comparing, we see that Qc=Kc=0.5
The reaction is already at equilibrium, hence there is no shift in the direction.
Theory:
Difference between equilibrium constant Keq and reaction quotient Q :
Keq (Equilibrium Constant)
The concentrations represented in the ratio are at equilibrium
Rate of forward Reaction = Rate of Backward Reaction.
Q (Reaction Quotient)
The concentrations represented in the ratio may or may not be at equilibrium
Rate of forward Reaction may or may not be equal to Rate of Backward Reaction.