Write a relation between ∆G and Q and define the meaning of each term and answer the following :
(a) Why a reaction proceeds forward when Q < K and no net reaction occurs when Q = K.
(b) Explain the effect of increase in pressure in terms of reaction quotient Q. for the reaction :
CO (g) + 3H2 (g)
⇌ CH4 (g) + H2O (g)
Write a relation between ∆G and Q and define the meaning of each term and answer the following :
(a) Why a reaction proceeds forward when Q < K and no net reaction occurs when Q = K.
(b) Explain the effect of increase in pressure in terms of reaction quotient Q. for the reaction :
CO (g) + 3H2 (g) ⇌ CH4 (g) + H2O (g)
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1 Answer
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This is a Long Answer Type Questions as classified in NCERT Exemplar
Ans: (a) As we know,
ΔG= ?G? +RTlnQ
?G? = Change in free energy as the reaction proceeds,
ΔG = Standard free energy change,
Q = Reaction quotient,
R = Gas constant,
T = Absolute temperature.
Since, ?G? =−RTlnK
∴ΔG=−RTlnK + RTlnQ = RTlnKQ?
If Q
If Q=K, ΔG=0, reaction is in equilibrium and no net reaction is there.
(b) When we increase the pressure equilibrium will shift in forward direction it means Q
Types of Chemical Reactions :
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