Addition of Inert Gas at Constant Pressure
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Q.
What happens to equilibrium when pressure is increased?
Q. Introduction of inert gas (at the same temperature) will affect the equilibrium if:
- Volume is constant and △ng≠0
- Pressure is constant and △ng≠0
- Volume is constant and △ng=0
- Pressure is constant and △ng=0
Q.
Unit of equilibrium constant for the reversible reaction
H2 + I2 ⇌ 2HI is
mol-1 litre
mol litre-1
Dimensionless
mol-2 litre
Q. The reaction between Cr2O2−7 and HNO2 in an acidic medium is :
Cr2O2−7+5H++3HNO2→2Cr3++3NO−3+4H2O
The rate of disappearance of Cr2O2−7 is found to be 2.4×10−4 molL−1s−1 during a measured time interval. Find the rate of disappearance of HNO2 and the rate of appearance of Cr3+ during this time interval respectively.
Cr2O2−7+5H++3HNO2→2Cr3++3NO−3+4H2O
The rate of disappearance of Cr2O2−7 is found to be 2.4×10−4 molL−1s−1 during a measured time interval. Find the rate of disappearance of HNO2 and the rate of appearance of Cr3+ during this time interval respectively.
- 7.2×10−4molL−1s−1 and 4.8×10−4molL−1s−1
- 4.8×10−4molL−1s−1 and 7.2×10−4molL−1s−1
- 2.4×10−4molL−1s−1 and 2.4×10−4molL−1s−1
- 4.8×10−4molL−1s−1 and 2.4×10−4molL−1s−1
Q. At constant pressure, which of the following is true for dissociation of PCl5(g) for the addition of inert gases?
- Reduces the dissociation of PCl5
- Does not affect the degree of dissociation of PCl5
- Increases the dissociation of PCl5
- Decrease in the formation of PCl3(g)
Q. Consider the following reaction in which dissociation of PCl5 (g) takes place:
PCl5 (g)⇌PCl3 (g)+Cl2 (g)
At a constant pressure, an inert gas Helium is added.
Which of the following statement is correct?
PCl5 (g)⇌PCl3 (g)+Cl2 (g)
At a constant pressure, an inert gas Helium is added.
Which of the following statement is correct?
- The dissociation of PCl5 increases.
- The dissociation of PCl5 decreases.
- Decrease in the formation of PCl3
- Does not affect the degree of dissociation of PCl5
Q. Consider a reaction:
2A (g)+3B (g)⇌3C (g)+2D (g)
When the pressure is increased :
2A (g)+3B (g)⇌3C (g)+2D (g)
When the pressure is increased :
- Equilibrium is shifted in forward direction
- Equilibrium is shifted in backward direction
- No change in equilibrium.
- 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
![](https://search-static.byjusweb.com/question-images/byjus/ckeditor_assets/pictures/932235/original_BPTL_NEET286th_Dec29_15.png)
![](https://search-static.byjusweb.com/question-images/byjus/ckeditor_assets/pictures/932235/original_BPTL_NEET286th_Dec29_15.png)
- increases
- decreases
- remains same
- changes unpredictably
Q. Consider the following equilibria:
(1) N2(g)+3H2(g)⇌2NH3(g)
(2) N2(g)+O2(g)⇌2NO(g)
(3) PCl5(g)⇌PCl3(g)+Cl2(g)
Choose the correct statement(s):
(1) N2(g)+3H2(g)⇌2NH3(g)
(2) N2(g)+O2(g)⇌2NO(g)
(3) PCl5(g)⇌PCl3(g)+Cl2(g)
Choose the correct statement(s):
- Addition of inert gas has no effect on all the three equilibria at constant temperature and also at constant pressure.
- Addition of an inert gas at constant volume has no effect on equilibria in (2).
- Addition of an inert gas at constant pressure favours the forward reaction in (3), backward reaction in (1) and has no effect on (2).
- 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 2.1×108, then at equilibrium the system will contain:
- Mostly products
- Similar amounts of reactants and products
- All reactants
- Mostly reactant
Q. If the intermolecular forces vanish away, the volume occupied by the molecules contained in 4.5 kg water at 0∘C and 1 atm will be given by:
- 4.5 m3
- 5.6 m3
- 11.2 m3
- 11.2 litre
Q. Consider a reaction:
2A (g)+3B (g)⇌3C (g)+2D (g)
When the pressure is increased :
2A (g)+3B (g)⇌3C (g)+2D (g)
When the pressure is increased :
- No change in equilibrium.
- Equilibrium is shifted in backward direction
- Equilibrium is shifted in forward direction
- None of the above
Q. Consider the following data:
ΔHfo(N2H4, l)=50kJ/mol, ΔHfo(NH3, g)=−46kJ/mol
B.E.(N−H)=393kJ/mol, B.E.(H−H)=436kJ/mol
ΔvapH(N2H4, l)=18kJ/mol
The N−N bond energy in N2H4 is:
ΔHfo(N2H4, l)=50kJ/mol, ΔHfo(NH3, g)=−46kJ/mol
B.E.(N−H)=393kJ/mol, B.E.(H−H)=436kJ/mol
ΔvapH(N2H4, l)=18kJ/mol
The N−N bond energy in N2H4 is:
- 226 kJ/mol
- 154 kJ/mol
- none of the above
- 190 kJ/mol
Q. At constant pressure, which of the following is true for dissociation of PCl5(g) for the addition of inert gases?
- Reduces the dissociation of PCl5
- Increases the dissociation of PCl5
- Does not affect the degree of dissociation of PCl5
- Decrease in the formation of PCl3(g)
Q. For the reaction: CO(g)+2H2(g)⇌CH3OH(g), find the equilibrium constant Kp if Kc=2500 at temperature 600 K?
- 4.92
- 2.04
- 1.03
- None of the above
Q.
Given the following reaction at equilibrium N2(g)+3H2(g)⇌2NH3(g). Some inert gas at constant pressure is added to the system. Which one of the following will happen?
More NH3(g) is produced
Less NH3(g) is produced
No effect on the equilibrium
Kp of the reaction is decreased
Q. Consider a reaction,
A(g)+B2(g)⇌AB2(g)
If the concentration of the reactants are doubled, then the equilibrium constant will:
A(g)+B2(g)⇌AB2(g)
If the concentration of the reactants are doubled, then the equilibrium constant will:
- Also be doubled
- Be halved
- Become one-fourth
- Remain the same
Q. Introduction of inert gas (at the same temperature) will affect the equilibrium if:
- Volume is constant and △ng≠0
- Pressure is constant and △ng≠0
- Volume is constant and △ng=0
- Pressure is constant and △ng=0
Q. When an inert gas is added to the given reversible process then the equilibrium:
- shift in forward direction
- cannot be predicted
- be unaffected
- shift in backward direction
Q. For the reaction, C(s)+H2O(g)⇌H2(g)+CO(g), by increasing pressure following equilibrium :
- remain unaffected
- proceed in backward direction
- proceed in forward direction
- 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.
If true enter 1, if false enter 0.
Q. For the homogeneous reaction 4NH3(g)+5O2(g)⇋4NO(g)+6H2O(g) the equilibrium constant Kc has the unit of:
- (conc)−1
- conc
- (conc)+10
- it is dimensionless
Q. Consider the reactions
(i) PCl5(g)⇌PCl3(g)+Cl2(g)
(ii) N2O4(g)⇌2NO2(g)
The addition of an inert gas at constant pressure:
(i) PCl5(g)⇌PCl3(g)+Cl2(g)
(ii) N2O4(g)⇌2NO2(g)
The addition of an inert gas at constant pressure:
- Will reduce the dissociation of PCl5 as well as N2O4
- Will increase the dissociation of PCl5 as well as N2O4
- Will increase the dissociation of PCl5 and step up the formation of NO2
- 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 :
- same as initial
- none of these
- half of initial
- 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.
If true enter 1, if false enter 0.
Q. Assertion :0.1M KCl, 0.1M K2SO4 solutions cause the same osmotic pressure in solution. Reason: Osmotic pressure depends on the number of particles present in the solution.
- Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
- Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
- Assertion is correct but Reason is incorrect
- Assertion is incorrect but Reason is correct
Q.
As pressure is increased, what will happen to the following reactions?
Match the column:Column - I | Column - II |
(P) PCl5(g)⇌PCl3(g)+Cl2(g) | (1) Shift to forward |
(Q) 2NO2(g)⇌N2O4(g) | (2) Shift to backward |
(R) H2(g)+I2(g)⇌2HI(g) | (3) No effect |
(S) aA(g)+bB(g)⇌cC(g) | (4) Cannot predict |
- 2 1 3 4
- 1 2 3 4
- 2 1 4 3
- 4 3 1 2
Q. Consider a reaction:
2A (g)+3B (g)⇌3C (g)+2D (g)
When the pressure is increased :
2A (g)+3B (g)⇌3C (g)+2D (g)
When the pressure is increased :
- Equilibrium is shifted in forward direction
- Equilibrium is shifted in backward direction
- No change in equilibrium.
- None of the above
Q. Consider the reactions
(i) PCl5(g)⇌PCl3(g)+Cl2(g)
(ii) N2O4(g)⇌2NO2(g)
The addition of an inert gas at constant volume:
(i) PCl5(g)⇌PCl3(g)+Cl2(g)
(ii) N2O4(g)⇌2NO2(g)
The addition of an inert gas at constant volume:
- will increase the dissociation of PCl5 and step up the formation of NO2
- will reduce the dissociation of PCl5 as well as N2O4
- will increase the dissociation of PCl5 as well as N2O4
- will not disturb the equilibrium of the reactions
Q.
Given the following reaction at equilibrium N2(g)+3H2(g)⇌2NH3(g). Some inert gas at constant pressure is added to the system. Which one of the following will happen?
No effect on the equilibrium
More
is produced
Less
is produced
of the reaction is decreased