Dynamic Nature of Physical and Chemical Equilibrium

Q.

What factors affect the equilibrium constant?

Q.

The spin multiplicity of nitrogen in the ground state.

Q. Chemical equilibrium is dynamic in nature because:

1. Equilibrium is maintained rapidly
2. The concentration of reactants and products becomes the same at equilibrium
3. The concentration of reactants and products are different at equilibrium
4. Both forward and backward reactions occur with the same speed at all times

Q.

Phosphorus pentachloride dissociates as follows, in a closed reaction vessel, ${\mathrm{PCl}}_5\rightleftharpoons {\mathrm{PCl}}_3\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$. If the total pressure at the equilibrium of the reaction mixture is $\mathrm{P}$ and the degree of dissociation of ${\mathrm{PCl}}_5$​ is $\mathrm{x}$, the partial pressure of ${\mathrm{PCl}}_3$​ will be:

Q.

Is the any way to find out whether a reaction is reversible or irreversible reaction?

Q. What do you mean by dynamic equilibrium!

Q. In a certain reaction, 10$\%$ of the reactant decomposes in 1 hr, 20 $\%$ in two hours, 30$\%$ in three hours and so on the dimensions of the rate constant is

1. $hou{r}^{-1}$
2. $molelitr{e}^{-1}se{c}^{-1}$
3. $litremol{e}^{-1}se{c}^{-1}$
4. $molese{c}^{-1}$

Q.

What are the types of equilibrium?

Q. Statement 1: Physical equilibrium is not static but dynamic in nature.
Satement 2: Physical equilibrium is a state in which two opposing processes are proceeding at the same rate.

1. Both statements are false
2. Satement 1 is false while Statement 2 is true.
3. Satement 1 is true while Statement 2 is false.
4. Both statements are true

Q. Statement 1: The chemical equilibrium is not static but dynamic in nature.
Statement 2: The chemical equilibrium is a state in which two opposing process(reactions) are producing at the same rate.

1. Both Statement 1 and Statement 2 are true and Statement 2 is the correct explanation of statement 1.
2. 
   Statement 1 is true but Statement 2 is false
3. Both Statement 1 and Statement 2 are true and Statement 2 is not the correct explanation of statement 1.
4. 
   Statement 1 is false but Statement 2 is true

Q. Which of the following statement is incorrect?

1. In an irreversible reaction, the reaction proceeds in one direction only
   
2. In an equilibrium mixture of ice and water kept in a perfectly insulated flask, the amount of ice and water remains constant
3. In a dynamic equilibrium, the reaction stops
4. At equilibrium there is no change in the concentration of either the reactants or the products

Q. Rate of a catalysed and an uncatalysed reaction can be equal if

1. Both reaction temperature are equal
2. Temperature of the uncatalysed reaction is more than the catalysed reaction
3. Temperature of the uncatalysed reaction is less than the catalysed reaction
4. Rate of catalysed reaction cannot be equal to uncatalysed reaction in any case.

Q.

The collision among the particles in a liquid causes it to evaporate.

1. True
2. False

Q. Which information can be obtained from Le Chatelier's principle?

1. Shift in equilibrium position on changing $P,T$ and concentration
2. Dissociation constant of a weak acid
3. Energy change in a reaction
4. Equilibrium constant of a chemical reaction

Q. One mole of $N_2{O}_4$ at 300 K is kept in a closed container under one atmosphere. It is heated to 600K when $20\%$ by mass of $N_2{O}_4$ decomposes to $N{O}_2$ ( g ) . The resultant pressure is :

1. 1.2 atm
2. 2.4 atm
3. 2.0 am
4. 1.0 atm

Q. In haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end?

1. 20 litres ammonia, 25 litres nitrogen, 15 litres hydrogen
2. 20 litres ammonia, 20 litres nitrogen, 20 litres hydrogen
3. 10 litres ammonia, 25 litres nitrogen, 15 litres hydrogen
4. 20 litres ammonia, 10 litres nitrogen, 30 litres hydrogen

Q. For the dissociation reaction
$N_2{O}_4\left(g\right)\rightleftharpoons 2N{O}_2\left(g\right)$. The degree dissociation (1) in terms of $K_p$ and total equilibrium pressure is:

1. $\alpha =\sqrt{\frac{4P+K_p}{K_p}}$
2. $\alpha =\sqrt{\frac{K_p}{4P}}$
3. none of these
4. $\alpha =\sqrt{\frac{K_p}{4P+K_p}}$

Q. In physical equilibrium, forces responsible for equilibrium are _______ in nature.

1. physical
2. chemical
3. strong
4. weak

Q. Write the rate law expression for the given equation N2O5= 2NO2+0.5O2

Q. $K_p$ for the reaction $A\rightleftharpoons B$ is 4. If initially only A is present then what will be the partial pressure of B after equilibrium?

<!--td {border: 1px solid #cccccc;}br {mso-data-placement:same-cell;}--> AIIMS 2016

1. 1
2. 1.2
3. 0.8
4. 0.6

Q. Statement 1: Physical equilibrium is not static but dynamic in nature.
Satement 2: Physical equilibrium is a state in which two opposing processes are proceeding at the same rate.

1. Satement 1 is false while Statement 2 is true.
2. Satement 1 is true while Statement 2 is false.
3. Both statements are true
4. Both statements are false

Q.

Assume ideal gas behaviour. For the reaction, $N_2{O}_5\left(g\right)\rightleftharpoons 2N{O}_2\left(g\right)+0.5O_2\left(g\right)$, the initial pressure is 600 mmHg and the pressure at any time is 960 mmHg. The fraction of $N_2{O}_5\left(g\right)$ decomposed at constant volume and temperature is:

1. 0.407

2. 0.549

3. 0.277

4. 0.113

Q.

Silver is a substance which expands on melting, so, its melting point______ when pressure is raised.

Q. At equilibrium which of the following reaction remains unaffected by pressure change?

1. $N_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2NO\left(g\right)$
2. $2S{O}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2S{O}_3\left(g\right)$
3. $2N{O}_2\left(g\right)\rightleftharpoons N_2{O}_4\left(g\right)$
4. $H_2\left(g\right)+I_2\left(g\right)\rightleftharpoons 2HI\left(g\right)$

Q. One mole of $N_2{O}_4\left(g\right)$ at 300 K is kept in a closed container under one atmosphere. It is heated to 600 K when 20% by mass of $N_{2}O\left(g\right)$ decomposes to $N{O}_2\left(g\right).$ The resultant pressure is

1. 1.0 atm
2. 1.2 atm
3. 2.4 atm
4. 2.0 atm

Q. In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expeced product. What will be the composition of gaseous mixture under the aforesaid condition in the end.

1. 20 litres ammonia, 25 litres nitrogen, 15 litres hydrogen
2. 20 litres ammonia, 20 litres nitrogen, 20 litres hydrogen
3. 10 litres ammonia, 25 litres nitrogen, 15 litres hydrogen
4. 20 litres ammonia, 10 litres nitrogen, 30 litres hydrogen

Q. $HI$ was heated in a sealed tube at ${440}^{o}C$ till the equilibrium was reached. $HI$ was found to be $22\%$ decomposed. The equilibrium constant for the dissociation of $HI$ is: $[2HI\rightleftharpoons H_2+I_2]$

1. $0.0796$
2. $0.0199$
3. $0.282$
4. $1.99$

Q. An increase in pressure in the reaction $2HI\left(g\right)\rightleftharpoons H_2\left(g\right)+I_2\left(g\right)$ would :

1. produce more $I^{-}\left(aq\right)$
2. produce more $H_2$
3. not effect the system
4. drive it to the right

Q. $K_{sp}$ of $CuS,A{g}_{2}S,HgS$ are ${10}^{-31},{10}^{-44},{10}^{-54}$ respectively. Select the correct order for their solubility in water:

1. $HgS>CuS>A{g}_{2}S$
2. $HgS>A{g}_{2}S>CuS$
3. $A{g}_{2}S>HgS>CuS$
4. $A{g}_{2}S>CuS>HgS$

Q. What is not something that a phase equilibrium line shows?

1. The equilibrium point between liquid and solid
2. The equilibrium point between liquid and gas
3. The equilibrium point between solid and liquid
4. The equilibrium point between solid and gas
5. The equilibrium point between gas and vapor