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.

Answer 1

As we know,  ΔG= ΔG^Θ + RT lnQ

ΔG^Θ = Change in free energy as the reaction proceeds,

ΔG = Standard free energy change,

Q = Reaction quotient,

R = Gas constant,

T = Absolute temperature.

Since, ΔG^Θ + 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.