NCERT Solutions for Chapter: Equilibrium, Exercise 1: Long Answer Type

How can you predict the following stage of a reaction by comparing the value of ${\mathrm{K}}_{\mathrm{c}}$ and ${\mathrm{Q}}_{\mathrm{c}}$?

Net reaction proceeds in the forward direction.

How can you predict the given stage of a reaction by comparing the values of ${\mathrm{K}}_{\mathrm{c}}$ and ${\mathrm{Q}}_{\mathrm{c}}$?

Net reaction proceeds in the backward direction. 

How can you predict the given stage of a reaction by comparing the value of ${\mathrm{K}}_{\mathrm{c}}$ and ${\mathrm{Q}}_{\mathrm{c}}$? 

No net reaction occurs.

On the basis of the Le Chatelier principle explain how temperature and pressure can be adjusted to increase the yield of ammonia in the following reaction.

${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right) \rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right) ∆\mathrm{H} =– 92.38 \mathrm{kJ} {\mathrm{mol}}^{–1}$

What will be the effect of the addition of argon to the above reaction mixture at constant volume? 

A sparingly soluble salt having general formula ${\mathrm{A}}_{\mathrm{x}}^{\mathrm{p}+}{\mathrm{B}}_{\mathrm{y}}^{\mathrm{q}-}$ and molar solubility $\mathrm{S}$ is in equilibrium with its saturated solution. Derive a relationship between the solubility and solubility product for such salt. 

Write a relation between $∆\mathrm{G}$ and $\mathrm{Q}$ and define the meaning of each term and answer Why a reaction proceeds forward when $\mathrm{Q}<\mathrm{K}$ and no net reaction occurs when $\mathrm{Q}=\mathrm{K}$? 

Write a relation between $∆\mathrm{G}$ and $\mathrm{Q}$ and define the meaning of each term and answer the following :

Explain the effect of an increase in pressure in terms of reaction quotient $\mathrm{Q}$. for the reaction : $\mathrm{CO}\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CH}}_4\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right)$