Addition of Inert Gas at Constant Pressure

Q.

What happens to equilibrium when pressure is increased?

Q. Introduction of inert gas (at the same temperature) will affect the equilibrium if:

1. Volume is constant and $△n_g\ne 0$
2. Pressure is constant and $△n_g\ne 0$
3. Volume is constant and $△n_g=0$
4. Pressure is constant and $△n_g=0$

Q.

Unit of equilibrium constant for the reversible reaction

$H_2+I_2\rightleftharpoons 2HI$ is

1. mol^-1 litre

2. mol litre^-1

3. Dimensionless

4. mol^-2 litre

Q. The reaction between $C{r}_2{O}_7^{2-}$ and $HN{O}_2$ in an acidic medium is :
$C{r}_2{O}_7^{2-}+5H^{+}+3HN{O}_2\to 2C{r}^{3+}+3N{O}_3^{-}+4H_{2}O$
The rate of disappearance of $C{r}_2{O}_7^{2-}$ is found to be $2.4\times {10}^{-4}\text{mol}{L}^{-1}{s}^{-1}$ during a measured time interval. Find the rate of disappearance of $HN{O}_2$ and the rate of appearance of $C{r}^{3+}$ during this time interval respectively.

1. $7.2\times {10}^{-4}\text{mol}{L}^{-1}{s}^{-1}$ and $4.8\times {10}^{-4}\text{mol}{L}^{-1}{s}^{-1}$
2. $4.8\times {10}^{-4}\text{mol}{L}^{-1}{s}^{-1}$ and $7.2\times {10}^{-4}\text{mol}{L}^{-1}{s}^{-1}$
3. $2.4\times {10}^{-4}\text{mol}{L}^{-1}{s}^{-1}$ and $2.4\times {10}^{-4}\text{mol}{L}^{-1}{s}^{-1}$
4. $4.8\times {10}^{-4}\text{mol}{L}^{-1}{s}^{-1}$ and $2.4\times {10}^{-4}\text{mol}{L}^{-1}{s}^{-1}$

Q. At constant pressure, which of the following is true for dissociation of $PC{l}_5$(g) for the addition of inert gases?

1. Reduces the dissociation of $PC{l}_5$
2. Does not affect the degree of dissociation of $PC{l}_5$
3. Increases the dissociation of $PC{l}_5$
4. Decrease in the formation of $PC{l}_3\left(g\right)$​

Q. Consider the following reaction in which dissociation of $PC{l}_5\left(g\right)$ takes place:
$PC{l}_5\left(g\right)\rightleftharpoons PC{l}_3\left(g\right)+C{l}_2\left(g\right)$
At a constant pressure, an inert gas Helium is added.
Which of the following statement is correct?

1. The dissociation of $PC{l}_5$ increases.
2. The dissociation of $PC{l}_5$ decreases.
3. Decrease in the formation of $PC{l}_3$
4. Does not affect the degree of dissociation of $PC{l}_5$

Q. Consider a reaction:
$2A\left(g\right)+3B\left(g\right)\rightleftharpoons 3C\left(g\right)+2D\left(g\right)$
When the pressure is increased :

1. Equilibrium is shifted in forward direction
2. Equilibrium is shifted in backward direction
3. No change in equilibrium.
4. None of the above

Q. Some quantity of water is contained in a container as shown in figure. As neon is added to this system at constnat pressure, the amount of liquid water in the vessel

1. increases
2. decreases
3. remains same
4. changes unpredictably

Q. Consider the following equilibria:
(1) $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$
(2) $N_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2NO\left(g\right)$
(3) $PC{l}_5\left(g\right)\rightleftharpoons PC{l}_3\left(g\right)+C{l}_2\left(g\right)$
Choose the correct statement(s):

1. Addition of inert gas has no effect on all the three equilibria at constant temperature and also at constant pressure.
2. Addition of an inert gas at constant volume has no effect on equilibria in (2).
3. Addition of an inert gas at constant pressure favours the forward reaction in (3), backward reaction in (1) and has no effect on (2).
4. Addition of an inert gas at constant pressure has no effect on equilibrium (2), but favours the forward reaction in (1) and backward reaction in (3).

Q. If the value of equilibrium constant for a particular reaction is $2.1\times {10}^8$, then at equilibrium the system will contain:

1. Mostly products
2. Similar amounts of reactants and products
3. All reactants
4. Mostly reactant

Q. If the intermolecular forces vanish away, the volume occupied by the molecules contained in $4.5kg$ water at $0^{\circ }C$ and $1atm$ will be given by:

1. $4.5m^3$
2. $5.6m^3$
3. $11.2m^3$
4. $11.2litre$

Q. Consider a reaction:
$2A\left(g\right)+3B\left(g\right)\rightleftharpoons 3C\left(g\right)+2D\left(g\right)$
When the pressure is increased :

1. No change in equilibrium.
2. Equilibrium is shifted in backward direction
3. Equilibrium is shifted in forward direction
4. None of the above

Q. Consider the following data:
$\Delta {H_f}^o(N_2{H}_4,l)=50kJ/mol,\Delta {H_f}^o({NH}_3,g)=-46kJ/mol$
$B.E.(N-H)=393kJ/mol,B.E.(H-H)=436kJ/mol$
$\Delta {}_{vap}H(N_2{H}_4,l)=18kJ/mol$
The $N-N$ bond energy in $N_2{H}_4$ is:

1. $226kJ/mol$
2. $154kJ/mol$
3. none of the above
4. $190kJ/mol$

Q. At constant pressure, which of the following is true for dissociation of $PC{l}_5$(g) for the addition of inert gases?

1. Reduces the dissociation of $PC{l}_5$
2. Increases the dissociation of $PC{l}_5$
3. Does not affect the degree of dissociation of $PC{l}_5$
4. Decrease in the formation of $PC{l}_3\left(g\right)$​

Q. For the reaction: $CO\left(g\right)+2H_2\left(g\right)\rightleftharpoons C{H}_{3}OH\left(g\right)$, find the equilibrium constant $K_p$ if $K_c=2500$ at temperature 600 K?

1. 4.92
2. 2.04
3. 1.03
4. None of the above

Q.

Given the following reaction at equilibrium $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$. Some inert gas at constant pressure is added to the system. Which one of the following will happen?

1. More $N{H}_3\left(g\right)$ is produced

2. Less $N{H}_3\left(g\right)$ is produced

3. No effect on the equilibrium

4. $K_p$ of the reaction is decreased

Q. Consider a reaction,
$A\left(g\right)+B_2\left(g\right)\rightleftharpoons A{B}_2\left(g\right)$
If the concentration of the reactants are doubled, then the equilibrium constant will:

1. Also be doubled
2. Be halved
3. Become one-fourth
4. Remain the same

Q. Introduction of inert gas (at the same temperature) will affect the equilibrium if:

1. Volume is constant and $△n_g\ne 0$
2. Pressure is constant and $△n_g\ne 0$
3. Volume is constant and $△n_g=0$
4. Pressure is constant and $△n_g=0$

Q. When an inert gas is added to the given reversible process then the equilibrium:

1. shift in forward direction
2. cannot be predicted
3. be unaffected
4. shift in backward direction

Q. For the reaction, $C\left(s\right)+H_{2}O\left(g\right)\rightleftharpoons H_2\left(g\right)+CO\left(g\right)$, by increasing pressure following equilibrium :

1. remain unaffected
2. proceed in backward direction
3. proceed in forward direction
4. cannot be predicted

Q. Addition of an inert gas at constant volume to the equilibrium mixture does not influence the equilibrium.
If true enter 1, if false enter 0.

Q. For the homogeneous reaction $4N{H}_3\left(g\right)+5O_2\left(g\right)\leftrightharpoons 4NO\left(g\right)+6H_{2}O\left(g\right)$ the equilibrium constant $K_c$ has the unit of:

1. $(conc{)}^{-1}$
2. $conc$
3. $(conc{)}^{+10}$
4. it is dimensionless

Q. Consider the reactions
(i) $PC{l}_5\left(g\right)\rightleftharpoons PC{l}_3\left(g\right)+C{l}_2\left(g\right)$
(ii) $N_2{O}_4\left(g\right)\rightleftharpoons 2N{O}_2\left(g\right)$
The addition of an inert gas at constant pressure:

1. Will reduce the dissociation of $PC{l}_5$ as well as $N_2{O}_4$
2. Will increase the dissociation of $PC{l}_5$ as well as $N_2{O}_4$
3. Will increase the dissociation of $PC{l}_5$ and step up the formation of $N{O}_2$
4. Will not disturb the equilibrium of the reactions

Q. Equal volumes of two isotonic solutions are mixed. The osmotic pressure of the final mixture is :

1. same as initial
2. none of these
3. half of initial
4. twice of initial

Q. High pressure is favourable for those reversible reactions in which there is decrease in the number of molecules.
If true enter 1, if false enter 0.

Q. Assertion :$0.1MKCl,0.1M{K}_2{SO}_4$ solutions cause the same osmotic pressure in solution. Reason: Osmotic pressure depends on the number of particles present in the solution.

1. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
2. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
3. Assertion is correct but Reason is incorrect
4. Assertion is incorrect but Reason is correct
   

Q. Match the column:

Column - I	Column - II
(P) $PC{l}_5\left(g\right)\rightleftharpoons PC{l}_3\left(g\right)+C{l}_2\left(g\right)$	(1) Shift to forward
(Q) $2N{O}_2\left(g\right)\rightleftharpoons N_2{O}_4\left(g\right)$	(2) Shift to backward
(R) $H_2\left(g\right)+I_2\left(g\right)\rightleftharpoons 2HI\left(g\right)$	(3) No effect
(S) $aA\left(g\right)+bB\left(g\right)\rightleftharpoons cC\left(g\right)$	(4) Cannot predict

1. 2 1 3 4
2. 1 2 3 4
3. 2 1 4 3
4. 4 3 1 2

Q. Consider a reaction:
$2A\left(g\right)+3B\left(g\right)\rightleftharpoons 3C\left(g\right)+2D\left(g\right)$
When the pressure is increased :

1. Equilibrium is shifted in forward direction
2. Equilibrium is shifted in backward direction
3. No change in equilibrium.
4. None of the above

Q. Consider the reactions
(i) $PC{l}_5\left(g\right)\rightleftharpoons PC{l}_3\left(g\right)+C{l}_2\left(g\right)$
(ii) $N_2{O}_4\left(g\right)\rightleftharpoons 2N{O}_2\left(g\right)$
The addition of an inert gas at constant volume:

1. will increase the dissociation of $PC{l}_5$ and step up the formation of $N{O}_2$
2. will reduce the dissociation of $PC{l}_5$ as well as $N_2{O}_4$
3. will increase the dissociation of $PC{l}_5$ as well as $N_2{O}_4$
4. will not disturb the equilibrium of the reactions

Q.

Given the following reaction at equilibrium $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$. Some inert gas at constant pressure is added to the system. Which one of the following will happen?

1. No effect on the equilibrium

2. More is produced

3. Less is produced

4. of the reaction is decreased