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Question
Write a relation between ∆G and Q and define the meaning term and answer the following:
Why a reaction proceeds forward when Q < K and no net reaction occurs when Q = K.
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Solution
As we know, ΔG= ΔGΘ + RT lnQ
ΔGΘ = Change in free energy as the reaction proceeds,
ΔG = Standard free energy change,
Q = Reaction quotient,
R = Gas constant,
T = Absolute temperature.
Since, ΔGΘ + RT lnK
∴ ΔG = − RT lnK + RT lnQ = RT lnKQ
If Q < K, ΔG will be negative. Reaction proceeds in the forward.
If Q = K, ΔG = 0, reaction is in equilibrium and no net reaction is there.
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Write a relation between ∆G and Q and define the meaning term and answer the following:
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