Factors Affecting Equilibria

For the chemical reaction  $3\mathrm{X}\left(\mathrm{g}\right)+\mathrm{Y}\text{(g)}\rightleftharpoons {\mathrm{X}}_3\mathrm{Y}\left(\mathrm{g}\right)$ , the amount of  $X_{3}Y$ at equilibrium is affected by –

State Le Chatelier's principle and apply it to the following equilibria: ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right)-\mathrm{Heat}$.

State Le Chatelier's principle and apply it to the following equilibria: $2\mathrm{NO}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{N}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)+\mathrm{Heat}$.

State and explain Le Chatelier's principle. Apply the principle to the following equilibria:

$2{\mathrm{NH}}_3\rightleftharpoons {\mathrm{N}}_2+3{\mathrm{H}}_2-\mathrm{Heat}$.

State and explain Le Chatelier's principle. Apply the principle to the following equilibria:

$2{\mathrm{SO}}_2+{\mathrm{O}}_2\rightleftharpoons 2{\mathrm{SO}}_3+\mathrm{Heat}$.

How does a catalyst influence the equilibrium constant?

How is it possible to make reversible reaction irreversible?

What is the effect of a catalyst on the equilibrium? 

${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\iff 2{\mathrm{NH}}_3\left(\mathrm{g}\right)+21.8 \mathrm{k} \mathrm{cal}$. The increase in pressure will result in?

State and example Le Chatlier's principle? Discuss which factors can influence the equilibrium state?

State Le-chatelier's principle. Mention two ways by which the concentration of ${\mathrm{SO}}_3$ can be increased in the following reaction in a state of equilibrium.

$2{\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\iff 2{\mathrm{SO}}_3\left(\mathrm{g}\right)+\mathrm{Heat}$

State Le Chaterlier's principle. What is the effect of temperature on equilibrium of the following reaction?

$2{\mathrm{NO}}_2\iff {\mathrm{N}}_2{\mathrm{O}}_4 ; ∆\mathrm{H}=-57.2 \mathrm{kJ} {\mathrm{mol}}^{-1}$

Which of the following conditions will favour the formation of ammonia in the reaction

${\mathrm{N}}_2+3{\mathrm{H}}_2\to 2{\mathrm{NH}}_3 ∆\mathrm{H}=-\mathrm{ve}$

Esterification of a carboxylic acid with an alcohol in the presence of mineral acid as catalyst is a reversible reaction.

If one mole of ethanoic acid and one mole of ethanol are allowed to reach equilibrium at $298\mathrm{K}$, how many moles of ethyl ethanoate and ethanoic acid are present at equilibrium? (Assume ${\mathrm{K}}_{\mathrm{c}} = 4 \mathrm{at} 298\mathrm{K}$)

Esterification of a carboxylic acid with an alcohol in the presence of mineral acid as catalyst is a reversible reaction.

Suggest two things that can be done with the products formed to push the reaction in the forward direction.

The change in standard Gibbs energy for a reaction at equilibrium, e.g.,${\mathrm{PCl}}_5\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{PCl}}_3\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$, on addition of an inert gas at constant pressure and then at constant volume respectively are :

When the following reaction is at equilibrium and the volume of the container is decreased,
${\mathrm{COCl}}_{2\left(\mathrm{g}\right)}\to {\mathrm{CO}}_{\left(\mathrm{g}\right)}+{{\mathrm{Cl}}_2}_{\left(\mathrm{g}\right)}$