Equilibrium practice · Mixed difficulty

Statement-I: Ethyl chloride reacts with sodium ethoxide to from diethyl etber. Here ethoxide ion behaves as strong base.
Statement-II: $\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}$ is weak acid.

Prove that the pressure necessary to obtain $50 \%$ dissociation of $\mathrm{PCl}_5$ at $250^{\circ} \mathrm{C}$ is numerically three times of $K_p$.

Molar solubility of Zirconium phosphate is ‘S’ moles/litre. Solubility product of Zirconium phosphate $\left[ {Z{r_3}{{\left( {P{O_4}} \right)}_4}} \right]$ is

An amount of 3 moles of $\mathrm{N}_2$ and some $\mathrm{H}_2$ is introduced into an evacuated vessel. The reaction starts at $t=0$ and equilibrium is attained at $t=t_1$. The amount of ammonia at $t=2 t_1$ is found to be $34 \mathrm{~g}.$ It is observed that $\frac{w\left(\mathrm{N}_2\right)}{w\left(\mathrm{H}_2\right)}=\frac{14}{3}$ at $t=\frac{t_1}{3}$ and $t=\frac{t_1}{2}.$ The only correct statement is

The equilibrium constants of the following are.

${\mathrm{N}_2} + 3{\mathrm{H}_\mathrm{2}}\leftrightharpoons2\mathrm{N}{\mathrm{H}_3}\mathrm{ }{\mathrm{K}_1}$

${\mathrm{N}_\mathrm{2}}\mathrm{ + }{\mathrm{O}_\mathrm{2}}\leftrightharpoons\mathrm{2NO }{\mathrm{K}_2}$

${\mathrm{H}_\mathrm{2}}\mathrm{ + }\frac{\mathrm{1}}{\mathrm{2}}{\mathrm{O}_\mathrm{2}} \to {\mathrm{H}_\mathrm{2}}\mathrm{O }{\mathrm{K}_3}$

The equilibrium constant $(K)$ of the reaction

$2\mathrm{N}{\mathrm{H}_3}\mathrm{ + }\frac{5}{2}{\mathrm{O}_2}\overset K \leftrightarrows \mathrm{2NO + 3}{\mathrm{H}_2}\mathrm{O,}$ will be

Which will undergo cationic hydrolysis?

The pH of solution, whose hydrogen ion concentration is one mole per litre, will be:

Consider the following reaction:

$\begin{aligned} & \mathrm{CuO}(\mathrm{s})+\mathrm{H}_2(\mathrm{g}) \rightleftharpoons \mathrm{Cu}(\mathrm{s})+\mathrm{H}_2 \mathrm{O}(\mathrm{g}) ; \mathrm{K}_1=2 \times 10^{15} \\ & \mathrm{H}_2(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{g}) \rightleftharpoons \mathrm{H}_2 \mathrm{O}(\mathrm{g}) ; \mathrm{K}_2=5 \times 10^{22} \end{aligned}$

The equilibrium constant for the reaction : $\mathrm{CuO}(\mathrm{s}) \rightleftharpoons \mathrm{Cu}(\mathrm{s})+\frac{1}{2} \mathrm{O}_2(\mathrm{g})$ would be:

A sparingly soluble Iron (III) salt dissociates in solution as follows:

${Fe}_2 {X}_3(\mathrm{s}) \rightleftharpoons 2 {Fe}^{+3}(\mathrm{aq})+3 {X}^{2-}(\mathrm{aq})$

If the solubility product of the iron (III) salt is ${K}_{{sp}}$, then $\left[{Fe}^{+3}\right](\mathrm{aq})$ at equilibrium is:

Calculate the concentration of $\mathrm{OH}$ in the solution of base with $\mathrm{pH}=12.301$.

The rate constant for forward reaction and backward reaction of hydrolysis of ester are ${1.1 \times {{10}^{ - 2}}}$ and ${1.5 \times {{10}^{ - 3}}}$ per minute respectively. Equilibrium constant for the reaction is

$\mathrm{C}{\mathrm{H}_3}\mathrm{COO}{\mathrm{C}_2}{\mathrm{H}_5} + {\mathrm{H}_2}\mathrm{O}\;\leftrightharpoons\;\mathrm{C}{\mathrm{H}_3}\mathrm{COOH} + {\mathrm{C}_2}{\mathrm{H}_5}\mathrm{OH}$

Which of the following is a Bronsted acid as well as Bronsted base:

The equilibrium constant for the reaction ${Br}_2 \rightleftharpoons 2 {Br}$ at $500 {~K}$ and $700 {~K}$ are $1 \times 10^{-10}$ and $1 \times 10^{-5}$ respectively. The reaction is;

(A): Benzoic acid $\left(K_a=6.5 \times 10^{-5}\right)$ is stronger acid than acetic acid

$\left(K_a=1.74 \times 10^{-5}\right)$

(R): Larger the value of $K_a$, greater is the acidity.

Identify the correct order of acidic strength of $\mathrm{C}{\mathrm{O}_2},\mathrm{CuO},\mathrm{CaO},{\mathrm{H}_2}\mathrm{O}:$

The following equilibria are given :

$\begin{aligned} & {N}_2+3 {H}_2 \rightleftharpoons 2 {NH}_3 ; {K}_1 \\ & {~N}_2+{O}_2 \rightleftharpoons 2 {NO} ; {K}_2 \\ & {H}_2+\frac{1}{2} {O}_2 \rightleftharpoons {H}_2 {O} ; {K}_3 \end{aligned}$

The equilibrium constant of the reaction $2 {NH}_3+\frac{5}{2} {O}_2 \rightleftharpoons 2 {NO}+3 {H}_2 {O}$ in terms of ${K}_1, {~K}_2$ and ${K}_3$ is

$\mathrm{N}_2 \mathrm{O}_4$ is $50 \%$ dissociated into $\mathrm{NO}_2$ at equilibrium. The vapour density of the gaseous mixture at equilibrium is

A solution contains a mixture of $\mathrm{Ag}^{+}(0.10 \mathrm{~M})$ and $\mathrm{Hg}_2^{2+}(0.10 \mathrm{~M}),$ which are to be separated by selective precipitation. Calculate the maximum concentration of iodide ion at which one of them gets precipitated almost completely. What per cent of that metal ion is precipitated before the start of precipitation of second metal ion? $K_{\mathrm{sp}}(\mathrm{AgI})=8.5\times 10^{-17}$ and $K_{\text {sp }}\left(\mathrm{Hg}_2 \mathrm{I}_2\right)=2.5 \times 10^{-26}.$

Which of the following statements are correct?

(i) Ionic product of water $\left({K}_{{w}}\right)=\left[{H}^{+}\right]\left[{OH}^{-}\right]=10^{-14} {M}^2$

(ii) At $298 {~K}\left[{H}^{+}\right]=\left[{OH}^{-}\right]=10^{-7}$

(iii) ${K}_{{w}}$ does not depends upon temperature

(iv) Molarity of pure water $=55.55 \,{M}$

Statement-1: In acidic medium ${Zn}^{2+}$ is not precipitated by ${S}^{-2}$ ions. and

Statement-2: Common ion effect increases the concentration of ${S}^{-2}$ ions

For the reaction $2 \mathrm{~A}(\mathrm{~g})+\mathrm{B}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}_2(\mathrm{~g})$ the equilibrium constant $K_p$ at $300 \mathrm{~K}$ is 16.0 . The value of $\mathrm{K}_{\mathrm{p}}$ for $\mathrm{AB}_2(\mathrm{~g}) \rightleftharpoons \mathrm{A}(\mathrm{g})+\frac{1}{2} \mathrm{~B}_2(\mathrm{~g})$ is:

Calculate $\mathrm{pH}$ of solution obtained by mixing equal vol. of $0.02 \mathrm{~M} \, {HOCl} \,\, \& \, \, 0.2 \mathrm{~M} \, {CH}_3 {COOH}$ solution given that $\mathrm{K}_{\mathrm{a}_1}({HOCl})=2 \times 10^{-4}, \mathrm{~K}_{\mathrm{a}_2}\left({CH}_3 {COOH}\right)=2 \times 10^{-5}.$

How will increase of pressure affect the equation?

$\mathrm{C}\left( s \right) + {\mathrm{H}_2}\mathrm{O}\left( \mathrm{g} \right)\leftrightharpoons\mathrm{CO}\left( \mathrm{g} \right) + {\mathrm{H}_2}\left( \mathrm{g} \right)$

For the equilibrium

$\mathrm{A}(\mathrm{g})+2 \mathrm{~B}(\mathrm{~g}) \rightleftharpoons \mathrm{AB}_2(\mathrm{~g})$

the value of equilibrium constant at $300 \mathrm{k}$ is $3 \times 10^{-3} \mathrm{~mole}^{-2} \mathrm{~L}^2$ and value of equilibrium constant at $500 \mathrm{k}$ is $5 \times 10^{-5} \mathrm{~mol}^{-2} \mathrm{~L}^2$.

What is the sign of enthalpy change for this reaction

$100 \mathrm{~mL}$ of a solution contains $2 \mathrm{~g}$ of acetic acid and $3 \mathrm{~g}$ of sodium acetate providing ${K}_{{a}}=1.8 \times 10^{-5}$ then choose the correct option

Unit of equilibrium constant for the reversible reaction ${H}_2+{I}_2 \rightleftharpoons$ $2 {HI}$ is

$3 \mathrm{~mol}$ ammonia is heated in presence of $1 \mathrm{~mol}$ of neon. At equilibrium, the mole fraction of hydrogen is found to be 0.5. The value of $\left(K_C\right) \times(V)$ for $\mathrm{NH}_3(\mathrm{g}) \rightleftharpoons \frac{1}{2} \mathrm{N}_2(\mathrm{g})+\frac{3}{2} \mathrm{H}_2(\mathrm{g})$

$K_p$ has the value of $10^{-6} {~atm}^3$ and $10^{-4} {~atm}^3$ at $298 {~K}$ and $323 {~K}$ respectively for the reaction
${CuSO}_4 \cdot 3 {H}_2 {O}({s}) \rightleftharpoons {CuSO}_4({~s})+3 {H}_2 {O}({g})$

$\Delta_{{r}} H^{\circ}$ for the reaction is :

STATEMENT-1 : The gas phase reaction $\mathrm{PCl}_3(g)+\mathrm{Cl}_2(g) \rightleftharpoons \mathrm{PCl}_5(g)$ shifts to the right on increasing pressure.

STATEMENT-2 : When pressure increases, equilibrium shifts towards more number of moles.

$\mathrm{Ca}\left(\mathrm{HCO}_3\right)_2(s)$ decomposes as $\mathrm{Ca}\left(\mathrm{HCO}_3\right)_2(s) \longrightarrow \mathrm{CaCO}_3(s)+\mathrm{H}_2 \mathrm{O}(g)+\mathrm{CO}_2(g)$
Total pressure at equilibrium is found to be 0.12 bar. Thus $K_p$ is