Factors Affecting Equilibria

For the reaction, $2\mathrm{A}\left(\mathrm{g}\right)+\mathrm{B}\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{C}\left(\mathrm{g}\right), \mathrm{\Delta H}=+13.6 \mathrm{kJ}$, which of the following will increase the extent of the reaction at equilibrium?

The thermal dissociation equilibrium reaction of ${\mathrm{CaCO}}_3\left(\mathrm{s}\right)$ is studied under different conditions
${\mathrm{CaCO}}_3\left(\mathrm{s}\right)\rightleftharpoons \mathrm{CaO}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$

For this equilibrium reaction, the correct statement(s) is/ (are):

At the equilibrium of the reaction, $2 \mathrm{X} \left(\mathrm{g}\right) + \mathrm{Y} \left(\mathrm{g}\right)\rightleftharpoons {\mathrm{X}}_2\mathrm{Y} \left(\mathrm{g}\right)$, the number of moles of ${\mathrm{X}}_2\mathrm{Y}$ at equilibrium is affected by the

Consider the following reaction ${\mathrm{CaCO}}_{3( \mathrm{s})}\rightleftharpoons {\mathrm{CaO}}_{\left(\mathrm{s}\right)}+{\mathrm{CO}}_{2\left(\mathrm{g}\right)}$ in closed container at equilibrium. What would be the effect of addition of ${\mathrm{CaCO}}_3$ on the equilibrium concentration of ${\mathrm{CO}}_2$?

For the following reversible reaction,

${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\leftrightharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right); {\mathrm{\Delta H}}_{\mathrm{f}}=-92 \mathrm{kJ}/\mathrm{mol}.$

At the equilibrium of the reaction, $2 \mathrm{X} \left(\mathrm{g}\right) + \mathrm{Y} \left(\mathrm{g}\right)\rightleftharpoons {\mathrm{X}}_2\mathrm{Y} \left(\mathrm{g}\right)$, the number of moles of ${\mathrm{X}}_2\mathrm{Y}$ at equilibrium is affected by the

What would happen to a reversible dissociation reaction at equilibrium when an inert gas is added while the pressure remains unchanged? Here $∆\mathrm{n} >0$

The reaction ${\mathrm{N}}_2 \left(\mathrm{g}\right) + 3{\mathrm{H}}_2 \left(\mathrm{g}\right) \rightleftharpoons 2{\mathrm{NH}}_3 \left(\mathrm{g}\right)$ is in equilibrium. Now the reaction mixture is compressed to half the volume

Which of the following statements is incorrect with respect to the given spontaneous reaction?

In the given diagram, a cylinder is divided by partition $\mathrm{P}$. In compartment $\mathrm{A},$ two gases ${\mathrm{O}}_2$ and ${\mathrm{O}}_3$are in equilibrium with each other.

Which of the following reactions will not get affected on increasing the pressure?

For the chemical equilibrium, $2{\mathrm{NO}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right);\mathrm{\Delta H}=\; +14.6\mathrm{ }\mathrm{kcal}\mathrm{ }$ increase in temperature$:$

Consider the reaction equilibrium:

$\begin{array}{ccccc}\text{Ice}& \rightleftharpoons & \text{Water}& -& \text{x kcal}\\ \left(\text{Greater volume}\right)& & \left(\text{Lesser volume}\right)& & \end{array}$.

The favourable conditions for forward reaction are:

For the gas phase reaction,

${\mathrm{C}}_2{\mathrm{H}}_4\left(\mathrm{g}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)\leftrightharpoons {\mathrm{C}}_2{\mathrm{H}}_6\mathrm{};\mathrm{}[∆\mathrm{H}=-32.7\mathrm{kcal}]$

Carried out in a vessel, the equilibrium concentration of ${\mathrm{C}}_2{\mathrm{H}}_4$ can be increased by:

On increasing temperature, the equilibrium constant of exothermic and endothermic reactions, respectively:

For a reaction $\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{B}\left(\mathrm{g}\right)+\mathrm{C}\left(\mathrm{g}\right).\mathrm{ }{\mathrm{K}}_{\mathrm{p}}$ at ${400}^{\mathrm{o}}$ C is 1.5 $\times {10}^{-4}$ and ${\mathrm{K}}_{\mathrm{P}}$ at ${600}^{\mathrm{o}}\mathrm{ }\mathrm{C}$ is $6\times {10}^{-3}$ . Which statement is incorrect?

Which statement about the given reaction is incorrect?

${\mathrm{N}}_2+3{\mathrm{H}}_2\to 2\mathrm{N}{\mathrm{H}}_3\mathrm{ };\mathrm{∆}\mathrm{H}=-\mathrm{v}\mathrm{e}$

Statement - 1: $\mathrm{S}{\mathrm{O}}_{2\left(\mathrm{g}\right)}+\frac{1}{2}{\mathrm{O}}_{2\left(\mathrm{g}\right)}\mathrm{ }\mathrm{f}\mathrm{ }\mathrm{S}{\mathrm{O}}_{3\left(\mathrm{g}\right)}+\mathrm{h}\mathrm{e}\mathrm{a}\mathrm{t}$ Forward reaction is favoured at high temperature and low pressure.

Statement - 2: Reaction is exothermic in forward direction

Statement - $1$: A catalyst increases the equilibrium constant at any fixed temperature. Statement - $2$: By the uses of catalyst the rate of the reaction increases.