Types of Equillibrium

Q. Vapour density of the equilibrium mixture of the reaction $2N{H}_3\left(g\right)\rightleftharpoons N_2\left(g\right)+3H_2\left(g\right)$
is $6.0$. The Percent disssociation of ammonia gas is:

1. 13.88
2. 58.82
3. 41.66
4. None of these

Q. At high temperature, the following equilibrium exists in a mixture of carbon, oxygen and their compound:
$C\left(s\right)+O_2\left(g\right)\rightleftharpoons C{O}_2\left(g\right){Keq}_1={10}^{-2}$
$2C\left(s\right)+O_2\left(g\right)\rightleftharpoons 2CO\left(g\right){Keq}_2={10}^{-3}$
$C\left(s\right)+C{O}_2\left(g\right)\rightleftharpoons 2CO\left(g\right){Keq}_3=X$
$2CO\left(s\right)+O_2\left(g\right)\rightleftharpoons 2C{O}_2\left(g\right){Keq}_4=Y$
What is the value of $\frac{X}{Y}$?

Q.

The volume of a closed reaction vessel in which the equilibrium -

$2S{O}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2S{O}_3\left(g\right)$ sets is halved, Now -

1. The rates of forward and backward reactions will remain the same.

2. The equilibrium will not shift.

3. The equilibrium will shift to the right.

4. The rate of forward reaction will become more than that of reverse reaction and the equilibrium will shift

Q. In a chemical equilibrium $A+B\rightleftharpoons C+D$, when 1 mole of each reactant are mixed, 0.6 mole each of the product s are formed. The equilibrium constant is:

1. 
2. 
3. 
4. 

Q. $A\rightleftharpoons B(K_c=3),B\rightleftharpoons C(K_c=5),$
$C\rightleftharpoons D(K_c=2),$
From the given values of equilibrium constant for the above reactions, the value of equilibrium constant for $D\rightleftharpoons A$ will be.

1. 15
2. 0.3
3. 30
4. 0.03

Q. $N_2{O}_3$ on decomposition gives NO and $N{O}_2,$ they are found to be in equilibrium at 300 K. If the vapour density of such an equilibrium mixture is 23.75, calculate percentage by mass of $N_2{O}_3$ in the equilibrium mixture?

1. 80%
2. 60%
3. 40%
4. 20%

Q. When sulphur (in the form of $S_8$) is heated at temperature $T$, at equilibrium, the pressure of $S_8$ falls by $30\%$ from $1.0atm$, because $S_8\left(g\right)$ is partially converted into $S_2\left(g\right).$
Find the value of $K_p$ for this reaction $S_8\left(g\right)\rightleftharpoons 4S_2\left(g\right)$.

1. $2.96$
2. $6.14$
3. $4.28$
4. None of these

Q. Which of the following is an example of heterogeneous equilibrium?

1. $2S{O}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2S{O}_3\left(g\right)$
2. $C{H}_{3}COOH\left(aq\right)+C{H}_{3}C{H}_{2}OH\left(aq\right)\rightleftharpoons C{H}_{3}COOC{H}_{2}C{H}_3\left(aq\right)+H_{2}O\left(l\right)$
3. $3Fe\left(s\right)+4H_{2}O\left(g\right)\rightleftharpoons F{e}_3{O}_4\left(s\right)+4H_2\left(g\right)$
4. All of the above

Q. Which of the following equation is not involved in Solvay process

1. 
2. 
3. 
4. 

Q. The forward reaction proceeds towards near completion if the equilibrium constant of a reaction is:

1. 
2. 
3. 
4. 

Q.

When reaction is carried out at standard states, then the equilibrium constant will be

Q. The molecular weight of a gas which diffuse through a porous plug at 1/6 th of the speed of hydrogen under identical conditions is :

1. 64
2. 12
3. 36
4. 72

Q. The value of $K_P$ is $1\times {10}^{-3}{\text{atm}}^{-1}$ at $25{}^{\circ }\text{C}$ for the reaction $2NO\left(g\right)+C{l}_2\left(g\right)\rightleftharpoons 2NOCl\left(g\right).$ A flask contains $NO$ at $0.02\text{atm}$ and at $25{}^{\circ }\text{C}$. The mole of $C{l}_2$ that must be added if $1\%$ of the $NO$ is to be converted to $NOCl$ at equilibrium is $x\times {10}^{-5}$. The volume of the flask is such that $0.2$ mole of gas produces $1\text{atm}$ pressure at $25{}^{\circ }\text{C}$ (Ignore probable association of $NO$ to $N_2{O}_2$). Find the value of $x$.
(Given: $\frac{1}{(99{)}^2}\approx 1.02\times {10}^{-4}$)

Q. Which of the following reaction shows heterogeneous equilibrium?

1. $N_2\left(g\right)+3H_2\left(g\right)\leftrightharpoons 2N{H}_3\left(g\right)$
2. $CaC{O}_3\left(s\right)\leftrightharpoons CaO\left(s\right)+C{O}_2\left(g\right)$
3. $C{H}_{3}COOH\left(l\right)+C_2{H}_{5}OH\left(l\right)\leftrightharpoons C{H}_{3}COO{C}_2{H}_5\left(l\right)+H_{2}O\left(l\right)$
4. $N_2\left(g\right)+O_2\left(g\right)\leftrightharpoons 2NO\left(g\right)$

Q. Statement I: At equilibrium, the concentration of reactants and products remains constant.
Statement II: At equilibrium, the rates of the forward and reverse reactions are equal.

1. Statement I and Statement II are true and Statement II is correct explanation of Statement I
2. Statement I and Statement II are true and Statement II is not correct explanation of Statement I
3. Statement I is true and Statement II is false
   
4. Statement I is false and Statement I is true
   

Q. For $A\left(g\right)+B\left(g\right)\rightleftharpoons C\left(g\right)+D\left(g\right),$ the equilibrium constant is $K_1$ and for $C\left(g\right)+D\left(g\right)\rightleftharpoons A\left(g\right)+B\left(g\right),$ the equilibrium constant is $K_2.$ The correct relation between $K_1$ and $K_2$ is

1. $K_1\times K_2=1$
2. $K_1\times (K_2-1)=0$
3. $K_1/K_2=1$
4. All of these

Q. Catalysis can be classified into two groups - homogeneous and heterogeneous.
(a) What do you mean by homogeneous catalysis?
(b) Write one example for heterogeneous catalysis.

Q. Which of the following statements is NOT correct regarding chemical catalysts?

1. They are not consumed during the chemical reaction.
2. They cannot make nonspontaneous reactions occur.
3. They do not have to be the same phase as the reactant molecules.
4. They shift equilibrated reactions to the product's side.
5. Enzymes are biological catalysts.

Q. Following chemical reaction involves a homogeneous catalyst
$2S{O}_2\left(g\right)+O_2\left(g\right)\stackrel{NO\left(g\right)}{\to }2S{O}_3\left(g\right)$.

1. True
2. False

Q.

In ionic equilibrium, unless otherwise mentioned, we always deal with only dilute solutions where the solvent is water - True or false?

1. False

2. True

Q. For the reaction, $2S{O}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2S{O}_3\left(g\right)$
What is $K_c$ when the equilibrium concentration of $\left[S{O}_2\right]=0.60\text{M},\left[O_2\right]=0.82\text{M}and\left[S{O}_3\right]=1.90\text{M}$?

1. $12.229{\text{L mol}}^{-1}$
2. $24.5{\text{L mol}}^{-1}$
3. $36.0{\text{L mol}}^{-1}$
4. $2.67\times {10}^3{\text{L mol}}^{-1}$

Q. 28g of $N_2$ and 6g of $H_2$ were mixed. At equilibrium 17g of $N{H}_3$ was formed. The weight of $N_2$ and $H_2$ at equilibrium are _________ respectively.

1. 11g & zero
2. 19 & 3g
3. 14g & 3g
4. 11g & 3g

Q. The rates of diffusion of two gases $A$ and $B$ are in the ratio $1:4.$ If the ratio of their masses present in the mixture is $2:3$. Calculate the ratio of their mole fraction.

Q. Chemical equilibrium for a reversible change means for :

1. the forward reaction proceeds as fast as the backward reaction, i.e., velocity of opposing reaction is equal
2. dynamic equilibrium
3. no change in concentration of reaction species with time
4. none of the above

Q. In presence of a catalyst, what happens to the chemical equilibrium?

1. Energy of activation of the forward and backwards reactions are lowered by same amount.
2. Equilibrium amount is not disturbed.
3. Rates of forward and reverse reaction increase by the same factor.
4. More product is formed.

Q. A gaseous hypothetical chemical equation $2A\rightleftharpoons 4B+C$ is carried out in a closed vessel. The concentration of $B$ is found to be increase by $5\times {10}^3\text{mo}\text{l}.L^{\text{- 1}}.$ in $10$ seconds. The rate of appearance of $B$ is:

1. $5\times {10}^2\text{mol}{\text{L}}^{\text{- 1}}\text{se}{\text{c}}^{\text{- 1}}$
2. $5\times {10}^5\text{mol}{\text{L}}^{\text{- 1}}\text{se}{\text{c}}^{\text{- 1}}$
3. $6\times {10}^{-5}\text{mol}{\text{L}}^{\text{- 1}}\text{se}{\text{c}}^{\text{- 1}}$
4. $4\times {10}^{-4}\text{mol}{\text{L}}^{\text{- 1}}\text{se}{\text{c}}^{\text{- 1}}$

Q. In an equilibrium mixture containing $N_2{O}_4\left(g\right)$ and $N{O}_2\left(g\right)$ at a certain temperature, the $N{O}_2$ is found to be $25\%$ by volume. The molecular weight of the equilibrium mixture is:

1. $40.25$
2. $80.5$
3. $46.0$
4. $70.4$

Q. The number of equations corresponds to the heat of formation at 298K
$H_{2\left(g\right)}+B{r}_{2\left(l\right)}\to 2HB{r}_{\left(g\right)}{C}_{\left(diamond\right)}+2H_{2\left(g\right)}\to C{H}_{4\left(g\right)}{C}_{(graphite,s)}+2H_2\left(g\right)+\frac{1}{2}{O}_2\left(l\right)\to C{H}_{3}OH\left(l\right)H_{2\left(g\right)}+\frac{1}{2}{O}_{2\left(g\right)}\to H_2{O}_{\left(l\right)}{C}_{(graphite,s)}+3H_2\left(g\right)+\frac{1}{2}{O}_2\left(l\right)\to C_2{H}_{5}OH\left(l\right)\frac{1}{2}{N}_{2\left(g\right)}+\frac{3}{2}{H}_{2\left(g\right)}\to N{H}_{3\left(g\right)}{C}_{(graphite.s)}+O_{2\left(g\right)}\to C{O}_{2\left(g\right)}{C}_{\left(diamond\right)}+\frac{1}{2}{O}_{2\left(g\right)}\to CO\left(g\right)$ ___

Q.

For the reaction, $H_2$ (g) + $I_2\left)\right(g)\leftrightharpoons$ 2HI(g) which of the following holds good?

1. =

2. <

3. 

4. >