Characteristics of Equilibrium Constant

Q.

Which of the following are not ionic compounds?

1. $KCl$ and $HCl$

2. $NaCl$ and $KCl$

3. $CC{l}_4$ and $NaCl$

4. $HCl$ and $CC{l}_4$

Q. A $1.2\%$ solution of $NaCl$ is isotonic with $7.2\%$ solution of glucose. Calculate the van't Hoff factor of $NaCl$

1. $1.5$
2. $1.95$
3. $1.70$
4. $1.25$

Q. At ${87}^{o}C,$ the following equilibrium is established $H_2\left(g\right)+S\left(s\right)\rightleftharpoons H_{2}S\left(g\right);K_P=7\times {10}^{-2}$
If 0.50 mole of hydrogen and 1.0 mole of sulphur are heated to ${87}^{o}C$ in 1.0 L vessel, what will be the partial pressure of $H_{2}S$ at equilibrium?

1. 0.966 atm
2. 1.38 atm
3. 9.66 atm
4. 0.0327 atm

Q.

Assertion (A): Following is a balanced chemical equation for the action of steam on iron: $3\mathrm{Fe}\left(\mathrm{s}\right)+4{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\to {\mathrm{Fe}}_3{\mathrm{O}}_4\left(\mathrm{s}\right)+4{\mathrm{H}}_2\left(\mathrm{g}\right)$

Reason (R): The law of conservation of mass holds good for a chemical equation.

1. Both (A) and (R) are true and (R) is the correct explanation of the assertion (A).

2. Both (A) and (R) are true, but (R) is not the correct explanation of the assertion (A).

3. (A) is true, but (R) is false.

4. (A) is false, but (R) is true.

Q. In which of the following cases, the reaction goes farthest to completion?

1. $A\rightleftharpoons B(K={10}^3)$
2. $A+B\rightleftharpoons C+D(K=10)$
3. $P\rightleftharpoons Q(K={10}^{-2})$
4. $X+Y\rightleftharpoons XY(K={10}^{-1})$

Q.

Differentiate between Rhombic sulphur and Mono-clinic sulphur.

Q.

Which of the compound gives the most stable carbonium ion on dehydration?

1. ${\mathrm{CH}}_3\mathrm{OH}$

2. ${\mathrm{CH}}_3\mathrm{CHO}$

3. ${\left({\mathrm{CH}}_3\right)}_3\mathrm{COH}$

4. ${\mathrm{CH}}_2=\mathrm{CH}-{\mathrm{CH}}_2{\mathrm{CH}}_2\mathrm{OH}$

Q.

Assuming ideal behaviour, the magnitude of $\log K$ for the following reaction at $25°\mathrm{C}$ is $\mathrm{x}\times {10}^{-1}$. The value of $\mathrm{x}$ is (integer answer) -

$3\mathrm{CH}\equiv \mathrm{CH}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{C}}_6{\mathrm{H}}_6\left(\mathrm{l}\right)$

[given-$∆{}_{\mathrm{f}}\mathrm{G}^0\left(\mathrm{CH}\equiv \mathrm{CH}\right)=-2.04\times {10}^5\mathrm{J}{\mathrm{mol}}^{-1}$, $∆{}_{\mathrm{f}}\mathrm{G}^0\left({\mathrm{C}}_6{\mathrm{H}}_6\right)=-1.24\times {10}^5\mathrm{J}{\mathrm{mol}}^{-1}$, $\mathrm{R}=8.314\mathrm{J}{\mathrm{K}}^{-1}{\mathrm{mol}}^{-1}$]

Q. A solution is prepared by dissolving $0.6g$ of urea $\text{(molar mass}=60gmo{t}^{-1})and1.8g$ of glucose $\text{(molar mass}=180gmo{l}^{-1}in100mL$ of water at ${27}^{\circ }C$. The osmotic pressure of the solution is $(R=0.08206Latm{K}^{-1}mo{l}^{-1})$

1. $4.92atm$
2. $2.46atm$
3. $1.64atm$
4. $8.2atm$

Q. In a closed system: $A\left(s\right)\rightleftharpoons 2B\left(g\right)+3C\left(g\right),$ if the partial pressure of C is doubled, then partial preassure of B will be.

1. one-half of its original value
2. two times the orginal pressure
3. $\frac{1}{2\sqrt{2}}$ times the original value
4. $2\sqrt{2}$ times the original value

Q. Calculate the degree of dissociation of $HI$ as $2HI\rightleftharpoons H_2+I_2$ at $450{}^{o}C$ , if the equilibrium constant for the dissociation reaction is 0.263.

1. $0.688$
2. $0.326$
3. $0.454$
4. $0.253$

Q.

The ammonia ${\mathrm{NH}}_3$ released on the quantitative reaction of $0.6\mathrm{g}$ urea (${\mathrm{NH}}_2{\mathrm{CONH}}_2$) with Sodium hydroxide ($\mathrm{NaOH}$)can be neutralized by

1. $200\mathrm{ml}$of $0.2\mathrm{N}$$\mathrm{HCl}$

2. $200\mathrm{ml}$of $0.4\mathrm{N}\mathrm{HCl}$

3. $100\mathrm{ml}$of $0.1\mathrm{N}\mathrm{HCl}$

4. $100\mathrm{ml}$ of $0.2\mathrm{N}\mathrm{HCl}$

Q.

Assertion (A): Classical smog occurs in cold humid climate and it is acidic as well as reducing in nature. Reason (R): It is a mixture of smoke, fog and sulphur dioxide.

1. A is not correct but R is correct.

2. Both A and R are correct and R is the correct explanation of A.

3. Both A and R are correct but R is not the correct explanation of A.

4. A is correct but R are not correct.

Q.

Which of the following are not ionic compounds?

1. $KCl$

2. $HCl$

3. $CC{l}_4$

4. $NaCl$

Q. What is the role of catalyst in an equilibrium?

1. catalyst changes the equilibrium constant
2. catalyst do not change the equilibrium constant
3. catalyst affects the forward and backward reaction equally.
4. (b) and (c) above.

Q.

Consider a $70\%$ efficient hydrogen-oxygen cell working under the standard condition at $1$bar and $298$K. Its cell reaction is

${\mathrm{H}}_2\left(\mathrm{g}\right)+\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right.{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

The work derived from the cell on the consumption of $1.0\times {10}^{-3}$$\mathrm{mol}\mathrm{of}{\mathrm{H}}_2\left(\mathrm{g}\right)$ is used to compress $1.00\mathrm{mol}$ of a monoatomic ideal gas in a thermally insulated container. What is the change in the temperature (in $\mathrm{K}$) of the ideal gas?

The standard reduction potentials for the two half-cells are given below

${\mathrm{O}}_2\left(\mathrm{g}\right)+4{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+4{\mathrm{e}}^{-}\to 2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$, $E^0$ = $1.23V$

$2{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}\to {\mathrm{H}}_2\left(\mathrm{g}\right)$, $E^0$ = $0.00V$

Use $\mathrm{F}=96500{\mathrm{Cmol}}^{-1}$, $\mathrm{R}=8.314{\mathrm{Jmol}}^{-1}{\mathrm{K}}^{-1}$.

Q.

For a certain first order reaction $32\%$ of the reactant is left after $570\mathrm{s}.$ The rate constant of this reaction is _______$\times {10}^{-3}{\mathrm{s}}^{-1}.$

(Round off the nearest integer).

[Given : ${\log }_{10}2=0.301,\ln 10=2.303]$

Q. One of the reaction that takes place in producing steel from iron ore is the reduction of iron (II) oxide by carbon monoxide to give iron metal and $C{O}_2$.
$FeO\left(s\right)+CO\left(g\right)\rightleftharpoons Fe\left(s\right)+C{O}_2\left(g\right)$
$;K_p=0.265$ atm at 1050 K.
What are the equilibrium partial pressures of $CO$ and $C{O}_2$ respectively at 1050 K if the initial partial pressures are: $P_{CO}=1.4$ atm and $P_{C{O}_2}=0.80$ atm?

1. $P_{CO}=1.739\text{atm and}{P}_{C{O}_2}=0.461atm$
   
2. $P_{CO}=17.39\text{atm and}{P}_{C{O}_2}=0.461atm$
3. $P_{CO}=1.79\text{atm and}{P}_{C{O}_2}=0.46atm$
4. $P_{CO}=2.739\text{atm and}{P}_{C{O}_2}=1.461atm$
   

Q. For the reaction $H_2+I_2\rightleftharpoons 2HI$
The value of equilibrium constant is 9.0.
The degree of dissociation of HI will be?

1. 2
2. 2/5
3. 5/2
4. 1/2

Q.

Explain why pure liquids and solids can be ignored while writing the equilibrium constant expression?

Q. $1$ mole of $C{H}_{3}COOH$ and $1$ mole of $C_2{H}_{5}OH$ are taken in $1\text{L}$ flask, $50\%$ of $C{H}_{3}COOH$ is converted into ester as:
$C{H}_{3}COOH\left(l\right)+C_2{H}_{5}OH\left(l\right)\rightleftharpoons C{H}_{3}COO{C}_2{H}_5\left(l\right)+H_{2}O\left(l\right)$

There is $33\%$ conversion of $C{H}_{3}COOH$ into ester, if $C{H}_{3}COOH$ and $C_2{H}_{5}OH$ have been taken initially in molar ratio $x:1,$ find $x.$

Q. What is the role of catalyst in an equilibrium?

1. catalyst changes the equilibrium constant
2. catalyst do not change the equilibrium constant
3. catalyst affects the forward and backward reaction equally.
4. (b) and (c) above.

Q. A reaction was found to be second order with respect to the concentration of carbon monoxide. If the concentration of carbon monoxide is doubled, with everything else kept the same, the rate of reaction will be

1. Remains unchanged
2. Tripled
3. Increases by a factor of $4$
4. Doubled

Q. Mixture $X=0.02mol$ of $\left[Co\right(N{H}_3{)}_{5}S{O}_4]Br$ and $0.02mol$ of $\left[Co\right(N{H}_3{)}_{5}Br]S{O}_4$ was prepared in 2 litre of solution.
$\text{1 litre of mixture X+ excess}AgN{O}_3\to Y$
$\text{1 litre of mixture X + excess}BaC{l}_2\to Z$
Number of moles of Y and Z are

1. $0.01,0.01$
2. $0.02,0.01$
3. $0.01,0.02$
4. $0.02,0.02$

Q. For the following gaseous equilibria $X,YandZ$ at $300K$
$X:2S{O}_2+O_2\rightleftharpoons 2S{O}_3$
$Y:PC{l}_5\rightleftharpoons PC{l}_3+C{l}_2$
$Z:2HI\rightleftharpoons H_2+I_2$

The ratio of $K_p$ and $K_c$ in the increasing order will be:

1. X = Y = Z
2. X < Y < Z
3. X < Z < Y
4. Z < Y < X

Q. $N_2+3H_2\rightleftharpoons 2N{H}_3$, starting with one mole of nitrogen and 3 moles of hydrogen, at equilibrium 50% of each had reacted. If the equilibrium pressure is $P$, the partial pressure of hydrogen at equilibrium would be:

1. $\frac{P}{2}$
2. $\frac{P}{3}$
3. $\frac{P}{4}$
4. $\frac{P}{6}$

Q.

Calculate the partial pressure of carbon monoxide from the following data:

$CaC{O}_3\left(s\right)\stackrel{\Delta }{⟶}CaO\left(s\right)+C{O}_2\left(g\right);K_p=8\times {10}^{-2}$

$C{O}_2\left(g\right)+C\left(s\right)\to 2CO\left(g\right)K_p=2$

1. $0.2$
2. $0.4$
3. $1.6$
4. $4$

Q. For the reaction $H_2+I_2\rightleftharpoons 2HI$
The value of equilibrium constant is 9.0.
The degree of dissociation of HI will be?

1. 2
2. 2/5
3. 5/2
4. 1/2

Q. For an equilibrium reaction, the rate constants for the forward and backward reactions are $2.38\times {10}^{-4}{s}^{-1}$ and $8.15\times {10}^{-5}{s}^{-1}$ respectively. The equilibrium constant for the reaction is:

1. 0.342
2. 2.92
3. 0.292
4. 3.42

Q. For the hypothetical reactions, the equilibrium constant $\left(K\right)$ values are given:
$A\rightleftharpoons B;K_1=2B\rightleftharpoons C;K_2=4C\rightleftharpoons D;K_3=3$
The equilibrium constant for the reaction $A\rightleftharpoons D$ will be:

1. 48
2. 12
3. 6
4. 24