Write a relation between G and Q and define the meaning of each t… - Vidyadip

Question

Write a relation between $\triangle G$ 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 an increase in pressure in terms of reaction quotient Q for the reaction:
$
CO(g)+3 H_2(g) \rightleftharpoons CH_4(g)+H_2 O(g)
$

✓

Answer

a. We know that, $\Delta G=\Delta G^{\circ}+R T \ln Q$
Where,
$\Delta G^{\circ}=$ Change in free energy as the reaction proceeds
$\Delta G=$ Standard free energy change
$Q =$ Reaction quotient
$T =$ Absolute temperature
Also, $\Delta G^{\circ}=-R T \ln K$
$
\begin{aligned}
& \Rightarrow \Delta G=-R T \ln K+R T \ln Q \\
& \therefore \Delta G=R T \ln \frac{Q}{K}
\end{aligned}
$
If $Q < K , \Delta G$ will be negative. So, the reaction proceeds in the forward direction.
If $Q = K , \Delta G=0$, reaction will be at equilibrium.
b. Reaction:
$
CO(g)+3 H_2(g) \rightleftharpoons CH_4(g)+H_2 O(g)
$
On increasing the pressure equilibrium will shift in forward direction, it means $Q < K$.

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