Equilibrium practice · Mixed difficulty

Equivalent amounts of ${\mathrm{H}_2}\;\mathrm{and}\;{\mathrm{I}_2}$ are heated in a closed vessel till equilibrium is obtained. If 80% of the hydrogen can be converted to $\mathrm{H},\;\mathrm{the}\;{K_c}$ at this temperature is

The thermal dissociation of calcium carbonate showing heterogeneous equilibrium is
${CaCO}_3({~s}) \rightleftharpoons {CaO}({s})+{CO}_2({~g})$

For this reactions which of the following is/are true

(i) ${K}_{{c}}^{\prime}=\left[{CO}_2({~g})\right]$

(ii) ${Kp}={pCO}_2$

(iii) $\left[{CaCO}_3\right.$ (s)] and $[{CaO}({s})]$ are both constant

(iv) $\left[{CO}_2({~g})\right]$ is constant

The solubility of $\mathrm{Ca}{\mathrm{F}_2}$ in pure water is $2.3 \times {10^{ - 6}}\;\mathrm{mol }\;\mathrm{d}{\mathrm{m}^{ - 3}}$. Its solubility product will be

Conjugate base and conjugate acid of $HSO_4^ -$ respectively are

Dissociation constants of two acids HA and HB are $4 \times {10^{ - 10}}$ and $1.8 \times {10^{ - 5}}$ resp. Whose ${P^H}$ value will be higher for a given molarity

For the reaction in equilibrium,

I. $\mathrm{CO}(g)+\frac{1}{2} \mathrm{O}_2(g) \rightleftharpoons \mathrm{CO}_2(g)$

II. $2 \mathrm{CO}(g)+\mathrm{O}_2(g) \rightleftharpoons 2 \mathrm{CO}_2(g)$
$\begin{array}{cccccccccccccccccccc} {{\text{Equilibrium}}\,\,{\text{constant}}}&{{\text{Free}}\,\,{\text{energy}}\,\,{\text{charge}}} \\ {{K_1}}&{\Delta {G_1}} \\ {{K_2}}&{\Delta {G_1}} \end{array}$
Then

The solvent which is neither proton donor nor proton acceptor is called:

When ${NaNO}_3$ is heated in a closed vessel, oxygen is liberated and ${NaNO}_2$ is left behind, then which of the following statements is correct at equilibrium?

${NaNO}_3({~s}) \rightleftharpoons {NaNO}_2({~s})+\frac{1}{2} {O}_2({~g}), \Delta {H}=+{ve}$

A solution is 0.1 M in $C{l^ - }$ and 0.001 M in $CrO_4^{2 - }$. Solid $AgN{O_3}$ is gradually added to it. Assuming that the addition does not change in volume and ${K_{sp}}(AgCl) = 1.7 \times {10^{ - 10}}\,{M^2}$ and ${K_{sp}}(A{g_2}Cr{O_4}) = 1.9 \times {10^{ - 12}}\,{M^3}$
Select correct statement from the following

Equilibrium constants ${K_1}$ and ${K_2}$  for the following equilibria are related as :
$\mathrm{NO}\left( \mathrm{g} \right) + \frac{1}{2}{\mathrm{O}_2}\left( \mathrm{g} \right)\leftrightharpoons\mathrm{N}{\mathrm{O}_2}\left( \mathrm{g} \right);{K_1}$
$2\mathrm{N}{\mathrm{O}_2}\left( \mathrm{g} \right)\leftrightharpoons2\mathrm{NO}\left( \mathrm{g} \right) + {\mathrm{O}_2}\left( \mathrm{g} \right);{K_2}$

$\mathrm{pH}$ of a mixture of $1 \mathrm{M}$ benzoic acid $\left(\mathrm{p} K_a=4.20\right)$ and $1 \mathrm{M}\, {C}_6 {H}_5 {COONa}$ is 4.5 . In $300 \mathrm{~mL}$ buffer, benzoic acid is $[\log 2=0.3]$

In the reactions, $A + 2B\leftrightharpoons2C$, if 2 moles of $A$, 3.0 moles of $B$ and 2.0 moles of C are placed in a 2 L flask and the equilibrium concentration of $C$ is 0.5 mol/L, the equilibrium constant $\left( {{K_c}} \right)$ for the reactions is

Any precipitate is formed when

Blue colour disappears in which solution by passing ${SO}_2$

Consider the equilibrium

$CO(g) + 3H_2(g) \rightleftharpoons CH_4(g) + H_2O(g)$

If the pressure applied over the system increases by
two fold at constant temperature then

(A) Concentration of reactants and products
increases.

(B) Equilibrium will shift in forward direction.

(C) Equilibrium constant increases since concentration of products increases.

(D) Equilibrium constant remains unchanged as concentration of reactants and products remain same.

Choose the correct answer from the options given below:

The $pH$ of an aqueous solution of $\mathrm{C}{\mathrm{H}_3}\mathrm{COONa}$ of concentration $C\left( \mathrm{M} \right)$ is given by

At constant temperature in one litre vessel, when the reaction,

$2\mathrm{S}{\mathrm{O}_3}\left( \mathrm{g} \right)\;\leftrightharpoons\;2\mathrm{S}{\mathrm{O}_2}\left( \mathrm{g} \right) + {\mathrm{O}_2}\left( \mathrm{g} \right)$ is at equilibrium, the $\mathrm{S}{\mathrm{O}_2}$ concentration is $0.6\;M$, initial concentration of $\mathrm{S}{\mathrm{O}_3}$ is $1M$. The equilibrium constant is :

Equilibrium constant $({K})$ for the reaction ${Ni}({s})+4 {CO}({g}) \rightleftharpoons {Ni}({CO})_4({~g})$ can be written in terms of

(1) ${Ni}({s})+2 {CO}_2({~g})+2 {C}(\mathrm{s}) \rightleftharpoons {Ni}({CO})_4({~g})$; equilibrium constant $={K}_{{1}}$.

(2) ${CO}_2({~g})+{C}({s}) \rightleftharpoons 2 {CO}({g})$; equilibrium constant $={K}_2$.

What is the relation between ${K}, {K}_2$ and ${K}_2$ ?

How much water should be added to $300 \mathrm{~mL}$ of $0.2 \mathrm{M}$ solution of acetic acid $\left(K_a=1.8 \times 10^{-5}\right)$ to increase its degree of dissociation two times?

Urea is

Which of the following is a wrong statement about equilibrium state?

Which salt will give maximum pH in aqueous solution :

If $1\;M\;\mathrm{C}{\mathrm{H}_3}\mathrm{COONa}$ is added to $1\;M\;\mathrm{C}{\mathrm{H}_3}\mathrm{COOH}$

Methyl orange is an indicator in acid-alkali titration. It gives:

The percentage error in $\left[ {{\mathrm{H}^ + }} \right]$ made by neglecting the ionisation of water in $1.0 \times {10^{ - 6}}\;M\;\mathrm{NaOH}$ is:

The ${K_{sp}}$ of $\mathrm{PbC}{\mathrm{O}_3}$ and $\mathrm{MgC}{\mathrm{O}_3}$ are $1.5 \times {10^{ - 15}}$ and $1 \times {10^{ - 15}}$ respectively at $298\;K$. The concentration of $\mathrm{P}{\mathrm{b}^{2 + }}$ ions in a saturated solution containing $\mathrm{MgC}{\mathrm{O}_3}$ and $\mathrm{PbC}{\mathrm{O}_3}$ is:

Ostwald’s dilution law is applicable for

When $\mathrm{CaC}{\mathrm{O}_3}$ is heated at a constant temperature in a closed container, the pressure due to $\mathrm{C}{\mathrm{O}_2}$ produced will:

$2\,\,ICl \to {I_2} + C{l_2};Kc = 0.14$ Initial concentration of ICl is 0.6 M, then equilibrium concentration of ${I_2}$ is

A mixture of $\mathrm{H}_2$ and $\mathrm{I}_2$ (vapour) in molecular proportion 2 : 3 was heated at $440^{\circ} \mathrm{C}$ till the reaction

$\mathrm{H}_2(\mathrm{~g})+\mathrm{l}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{H}(\mathrm{g})$

reached equilibrium state. Calculate the percentage of $\mathrm{I}_2$ converted into HI. $\left(\mathrm{K}_{\mathrm{c}}\right.$ at $440^{\circ} \mathrm{C}$ is 0.02 and $\mathrm{x}$ is small compared to unity)