Embibe Experts Solutions for Chapter: Chemical Equilibrium, Exercise 1: EXERCISE

$4$ moles of ${\mathrm{PCl}}_5$ are heated at constant temperature in closed container. If degree of dissociation for ${\mathrm{PCl}}_5$ is $0.5$ calculate total number of moles at equilibrium.

For the reaction $3\mathrm{A} \left(\mathrm{g}\right)+\mathrm{B} \left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{C} \left(\mathrm{g}\right)$ at a given temperature, ${\mathrm{K}}_{\mathrm{c}}=9.0$. What must be the volume of the flask, if a mixture of $2.0 \mathrm{mol}$ each of $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$ exist in equilibrium?

$4.5$ moles each of hydrogen and iodine heated in a sealed ten litre vessel. At equilibrium, $3$ moles of $\mathrm{HI}$ were found. Determine the equilibrium constant for ${\mathrm{H}}_2 \left(\mathrm{g}\right)+{\mathrm{I}}_2 \left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{Hl} \left(\mathrm{g}\right)$.

$4$ moles of $\mathrm{A}$ are mixed with $4$ moles of $\mathrm{B}$, when $2$ moles of $\mathrm{C}$ are formed at equilibrium, according to the reaction, $\mathrm{A}+\mathrm{B}\rightleftharpoons \mathrm{C}+\mathrm{D}$. Determine equilibrium constant.

$\mathrm{A}\rightleftharpoons \mathrm{B}$. In this reaction, ${\mathrm{k}}_{\mathrm{f}}$ is $2\times {10}^{-3}$ and ${\mathrm{k}}_{\mathrm{b}}$ is $5\times {10}^{-4}$. Determine the value of ${\mathrm{K}}_{\mathrm{c}}$.

The equilibrium ${\mathrm{N}}_2 \left(\mathrm{g}\right)+{\mathrm{O}}_2 \left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO} \left(\mathrm{g}\right)$ established in a reaction vessel of $2.5 \mathrm{L}$ capacity. The amounts of ${\mathrm{N}}_2$ and ${\mathrm{O}}_2$ taken at the start were respectively $2$ moles and $4$ moles. Half a mole of nitrogen has been used up at equilibrium. What is the molar concentration of nitric oxide?

$2$ moles of ${\mathrm{PCl}}_5$ when heated in a closed vessel of $2$ litre capacity at equilibrium $40 \%$ of ${\mathrm{PCl}}_5$ dissociated in ${\mathrm{PCl}}_3$ and ${\mathrm{Cl}}_2$. What is the value of the equilibrium constant?

${\mathrm{K}}_{\mathrm{c}}=9$ for the reaction, $\mathrm{A}+\mathrm{B}\rightleftharpoons \mathrm{C}+\mathrm{D}$. If $\mathrm{A}$ and $\mathrm{B}$ are taken in equal amounts, then what is the amount of $\mathrm{C}$ in equilibrium?