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Question

For a reaction,
HCl (aq)+NaOH (aq)NaCl (aq)+H2O (l)Given Kc=0.5,[HCl]=3 M, [NaOH]=4 M,[NaCl]=6 M
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 C Qc=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.



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