Equilibrium practice · Hard

The following equilibrium constants were determined at $1120 {~K}$ :
$\begin{aligned} & 2 {CO}(g) \rightleftharpoons {C}({s})+{CO}_2({~g}) ; K_{p_1} =10^{-14} {~atm}^{-1} \\ & {CO}(g)+{Cl}_2(g) \rightleftharpoons {COCl}_2({~g}) ; K_{p_2} =6 \times 10^{-3} {~atm}^{-1} \end{aligned}$
What is the equilibrium constant $K_c$ for the following reaction at $1120 {~K}$ :
${C}({s})+{CO}_2({~g})+2 {Cl}_2({~g}) \rightleftharpoons 2 {COCl}_2({~g})$

Given,
$\mathrm{H}_2 \mathrm{~S}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(l)\rightleftharpoons\mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{HS}^{-}(\mathrm{aq})$; $K=9.1 \times 10^{-8}$ and for
$\mathrm{FeS}(s)+\mathrm{H}_2 \mathrm{O}(l)\rightleftharpoons\mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{HS}^{-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) ;$ $K=5 \times 10^{-19}$
Thus, molar solubility of $\mathrm{FeS}(s)$ in a buffer solution of $\mathrm{pH}=3.0$ in which $\left[\mathrm{H}_2 \mathrm{~S}\right]$ is fixed at $0.1 \mathrm{M}$, is

A vessel at 1000 K contains $\mathrm{C}{\mathrm{O}_2}$ with a pressure of 0.5 atm. Some of the $\mathrm{C}{\mathrm{O}_2}$ is converted into $\mathrm{CO}$ on the addition of graphite. If the total pressure at equilibrium is 0.8 atm, the value of ${K_p}$ is

Sulphide ion $\left(\mathrm{S}^{2-}\right)$ reacts with solid sulphur forming $\mathrm{S}_2^{2-}$ and $\mathrm{S}_3^{2-}$ with formation constants 12 and 132 . Formation constant of $\mathrm{S}_3^{2-}$ from sulphur and $\mathrm{S}_2^{2-}$ is

Find the value of $\mathrm{K}_{\mathrm{p}}$ for dissociation of:

$2 \mathrm{HI} \rightleftharpoons \mathrm{H}_2+\mathrm{I}_2$,

if the equilibrium concentration of $\mathrm{HI}, \mathrm{H}_2$ and $\mathrm{I}_2$ are $3.53,0.4789$ and $0.4789 \mathrm{~mole ~litre}^{-1}$ respectively.

Phenolphthalein can’t be used in the titration of

What is ${P^H}$ of 0.02 M solution of ammonium chloride at ${25^\mathrm{o}}C\,\,\,\,\left( {{K_b}\,\,\mathrm{ of }\,\,N{H_3} = 1.8 \times {{10}^{ - 5}}} \right)$

What is the minimum $\mathrm{pH}$ required to prevent the precipitation of $\mathrm{ZnS}$ in a solution that is $0.01 \mathrm{M} \,\, \mathrm{ZnCl}_2$ and saturated with $0.10 \mathrm{M} \,\, \mathrm{H}_2 \mathrm{~S}$ ?
[Given $\mathrm{K}_{\mathrm{sp}}=10^{-21}, \mathrm{~K}_{\mathrm{a}_1} \times \mathrm{K}_{\mathrm{a}_2}=10^{-20}$ ]

A solution of a weak monobasic acid has $\wedge_M$ for $0.1 N$ solution and $\wedge_{\infty}$ equal to $60 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ and $400 \mathrm{~S}$ $\mathrm{cm}^2 \mathrm{~mol}^{-1}$ respectively. The $\mathrm{pH}$ of this solution and $K_a$ of acid is :

For the following reactions, equilibrium constants are given: $S(s) + {O_2}(g)\underset{{}}{\overset{{}}{\leftrightharpoons}}S{O_2}(g);{K_1} = {10^{52}}$
$2S(s) + 3{O_2}(g)\leftrightharpoons2S{O_3}(g);{K_2} = {10^{129}}$
The equilibrium constant for the reaction, $2SO(g) + {O_2}(g)\leftrightharpoons2S{O_3}(g)$ is

Solubility of $\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2$ in $100 \mathrm{~ml}$ of pure water is $\mathrm{w~gm}$. Find out $\mathrm{k_{s p}}$ of $\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2\,(\mathrm{M}=$ molecular mass of $\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2)$

In an evacuated rigid vessel of volume $V$ litre, one mole of solid ammonium carbonate $\left(\mathrm{NH}_2 \mathrm{CONH}_4\right)$ is taken and the vessel is heated to $T \mathrm{~K}.$ The equilibrium total pressure of gases is found to be $P$ atm. The percentage dissociation of solid into $\mathrm{NH}_3(\mathrm{g})$ and $\mathrm{CO}_2(\mathrm{g})$ is

The degree of dissociation of acetic acid in a $0.1 \mathrm{~M}$ solution is $1.32 \times 10^{-2}.$ Calculate dissociation constant of acid and its $\text{pK}_\text{a}$ value:

The partial pressure of ethane over a solution containing $6.56 \times 10^{-3} \mathrm{~g}$ of ethane is $1\,\mathrm{bar}$. If the solution contains $5.00 \times 10^{-2} \mathrm{~g}$ of ethane, then what will be the partial pressure of gas?

The $\left[ {{\mathrm{H}^ + }} \right]$ ion concentration in $0.001\;M$ acetic acid is $1.34 \times {10^{ - 4}}\;\mathrm{g}\;\mathrm{ ion}\;/\mathrm{litre}\mathrm{.}$ The $\left[ {{\mathrm{H}^ + }} \right]$ ion concentration of $0.164\;\mathrm{g}\;\mathrm{ of}\;\mathrm{ C}{\mathrm{H}_3}\mathrm{COONa}$ is added to a litre of $0.001\;M$ $\mathrm{C}{\mathrm{H}_3}\mathrm{COOH}$ will be:

The equilibrium constant for the reversible reaction ${N}_{{2}}+3 {H}_{{2}} \rightleftharpoons 2 {NH}_3$ is $K$ and for reaction $\frac{1}{2} {N}_2+\frac{3}{2} {H}_2 \rightleftharpoons {NH}_3,$ the equilibrium constant is ${K}^{\prime}$

The $K$ and $K^{\prime}$ will be related as:

Ionisation of weak acid can be calculated by the formula

What is the molar solubility of $Al{\left( {OH} \right)_3}$ in 0.2 M NaOH solution? Given that, solubility product of $Al{\left( {OH} \right)_3} = 2.4 \times {10^{ - 24}}$

Given, $p K_b$ values
$\begin{array}{cccccccccccccccccccc} {{\text{Species}}}&{p{K_b}} \\ {N{H_3}}&{4.74} \\ {{A^ - }}&{4.00} \\ {{B^ - }}&{5.00} \\ {{C^ - }}&{6.00} \end{array}$
queous solutions of $0.01 \mathrm{M}$ salts of $\mathrm{HX}$

$(X=A, B, C)$ and $\mathrm{NH}_4 \mathrm{OH}$ have $\mathrm{pH}$ in the order

$\mathrm{I}_2+\mathrm{I}^{-} \rightleftharpoons \mathrm{I}_3^{-}$This reaction is set-up in aqueous medium. We start with 1 mole of $\mathrm{I}_2$ and 0.5 mole of $\mathrm{I}^{-}$in $1 \mathrm{~L}$ flask. After equilibrium is reached, excess of $\mathrm{AgNO}_3$ gave 0.25 mole of yellow precipitate. equilibrium constant is

The equilibrium $\mathrm{NH}_4 \mathrm{HS}(\mathrm{s}) \rightleftharpoons \mathrm{NH}_3(\mathrm{g})+\mathrm{H}_2 \mathrm{S}(\mathrm{g})$ is achieved at the equilibrium pressure of '$\mathrm{X}$' bar at $T \mathrm{~K}.$ The value of $\Delta_{\mathrm{r}} G^{\circ}$ for the reaction is

A $50 \mathrm{~ml}$ of mixture of $\mathrm{He}, \mathrm{CO}$ and $\mathrm{C}_2 \mathrm{H}_6$ was exploded in $120 \mathrm{~ml}$ of oxygen. On cooling, the gases occupied $142 \mathrm{~ml}$. After treatment with $\mathrm{KOH}$ the volume reduced by $26 \mathrm{~ml}$ and again on treatment with alkaline pyrogallol the volume further reduced, then wrong one is ___

The solubility of metal sulphide in saturated solution of $\mathrm{H}_2 \mathrm{S}$ (concentration $=0.1 \mathrm{~M}$) can be represented as follows.

$\mathrm{MS}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq}) \rightleftharpoons \mathrm{M}^{2+}(\mathrm{aq})+\mathrm{H}_2 \mathrm{S}(\mathrm{aq}) ; K_{\mathrm{eq}}=\frac{\left[\mathrm{M}^{2+}\right]\left[\mathrm{H}_2 \mathrm{S}\right]}{\left[\mathrm{H}^{+}\right]^2}$

The values of $K_{\mathrm{eq}}$ for the metal sulphides, $\text{MnS, } \mathrm{ZnS}, \mathrm{CoS}$ and $\mathrm{PbS}$ are $3 \times 10^{10}, 3 \times 10^{-2}, 3$ and $3\times 10^{-7},$ respectively. If the concentration of each metal ion in a saturated solution of $\mathrm{H}_2 \mathrm{S}$ is $0.01 \, \mathrm{M},$ then which metal sulphide(s) will precipitate at $\left[\mathrm{H}^{+}\right]=1.0 \mathrm{~M}?$

The solubility of ${AgCl}$ in water at $298 \mathrm{~K}$ is $1.06 \times 10^{-5} \text{ mol L}^{-1}.$ The solubility product of ${AgCl}$ at the same temperature was found to be ${p} \times 10^{-q}$. The values of ${p}$ and ${q}$ are respectively

$1 \mathrm{~mol}$ of ${N}_2$ and $4 \mathrm{~mol}$ of ${H}_2$ are allowed to react in a vessel to form ${NH}_3$ gas as only product and after reaction, water is added. Aqueous solution required $1 \mathrm{~mol}$ of ${HCl}$ for complete reaction. Mol fraction of ${H}_2$ in the gas mixture after reaction is

The solids dissociate as follows: $A\left( s \right)\,\leftrightharpoons\,B\left( g \right) + C\left( g \right);\,\,{K_{{P_1}}} = x\,\,\,\mathrm{at}{\mathrm{m}^2}$
$D\left( s \right)\,\leftrightharpoons\,C\left( g \right) + E\left( g \right);\,\,{K_{{P_2}}} = y\,\,\,\mathrm{at}{\mathrm{m}^2}$ The total pressure when both the solids dissociate simultaneously is

$K_1, K_2$ and $K_3$ are the equilibrium constants of the following reactions (I), (II) and (III) respectively:

(I) ${N}_2+2 {O}_2 \rightleftharpoons 2 {NO}_2$

(II) $2 {NO}_2 \rightleftharpoons {N}_2+2 {O}_2$

(III) ${NO}_2 \rightleftharpoons \frac{1}{2} {~N}_2+{O}_2$

The correct relation from the following is

Calculate the pH and degree of hydrolysis of $0.01 \mathrm{~M}$ solution of $\mathrm{NaCN}, \mathrm{K}_{\mathrm{a}}$ for $\mathrm{HCN}$ is $6.2 \times 10^{-12}.$

When heated ammonium carbamate decomposes as follows

${NH}_4 {COONH}_2\text{(s)} \Leftrightarrow 2 {NH}_3(\mathrm{g})+{CO}_2(\mathrm{g})$

At a certain temperature, the equilibrium pressure of the system is $0.318 \mathrm{~atm}, {K}_{{p}}$ for the reaction is

The normal vapor density of ${PCl}_5$ is 104.25. At $250^{\circ} \mathrm{C},$ its vapor density is 57.9. The degree of dissociation of ${PCl}_5$ at this temperature will be