R.C. Mukherjee Test: Chemical Equilibrium - NEET MCQ

The equilibrium constant for the given reaction :

SO₃(g)  SO₂(g) + O₂(g); K_c = 4.9 × 10^-2

The value of K_c for the reaction :

2SO₂(g) + O₂(g)  2SO₃(g), will be

For the following three reactions 1, 2 and 3, equilibrium constants are given :

(1) CO(g) + H₂O(g)CO₂(g)+H₂(g) ; K₁ 

(2) CH₄(g)+H₂O(g)CO(g)+3H₂(g) ; K₂

(3) CH₄(g)+2H₂O(g)CO₂(g)+4H₂(g) ; K₃

Which of the following relations is correct ?

Consider following reactions in equilbrium with equilibrium concentration 0.01M of every species

(I) PCl₅(g)  PCl₃(g) + Cl₂(g)

(II) 2HI(g)  H₂(g) + I₂(g)

(III) N₂(g) + 3H₂ (g)  2NH₃(g)

Extent of the reactions taking place is :

A definite amount of solid NH₄HS is placed in a flask already containing ammonia gas at a certain temperature and 0.50 atm pressure. NH₄HS decomposes to give NH₃ and H₂S and at equilibrium total pressure in flask is 0.84 atm. The equilibrium constant for the reaction is :

For the reaction 3A(g) + B(g)  2C(g) at a given temperature, K_c = 9.0. What must be the volume of the flask, if a mixture of 2.0 mol each of A, B and C exist in equilibrium ?

Sulfide ion in alkaline solution reacts with solid sulfur to form polysulfide ions having formulas S₂^2-, S₃^2-, S₄^2- and so on. The equilibrium constant for the formation of S₂^2- is 12 (K₁) & for the formation of S₃^2- is 132 (K₂), both from S and S^2-. What is the equilibrium constant for the formation of S₃^2- from S₂^2- and S

1 mole N₂ and 3 mol H₂ are placed in a closed container at a pressure of 4 atm. The pressure falls to 3 atm at the same temperature when the following equilibrium is attained.

N₂(g) + 3H₂(g)  2NH₃(g). The equilibrium constant K_p for dissociation of NH₃ is :

One mole of N₂O₄(g) at 300 K is left in a closed container under one atm. It is heated to 600 K when 20% by mass of N₂O₄ (g) decomposes to NO₂(g). The resultant pressure is :

For the following gases equilibrium. N₂O₄(g)  2NO₂(g) K_p is found to be equal to K_c. This is attained when temperature is

For the reaction :

CO(g) + O₂(g)  CO₂(g), K_p/K_c is :

For the reaction :

2NO₂(g)  2NO(g) + O₂(g) K_c = 1.8 × 10^-6 at 184°C and R = 0.083 JK^-1mol^-1. When K_p and K_c are compared at 184°C, it is found that :

PCl₅ dissociation a closed container as :

PCl₅(g)  PCl₃(g) + Cl₂(g)

If total pressure at equilibrium of the reaction mixture is P and degree of dissociation of PCl₅ is α, the partial pressure of PCl₃ will be :

For the reaction : 2HI (g)  H₂(g) + I₂(g), the degree of dissociated (α) of HI(g) is related to equilibrium constant K_p by the expression :

The equilibrium constant for the reaction

A(g) + 2B(g)  C(g) is 0.25 dm⁶ mol^-2. In a volume of 5 dm³, what amount of A must be mixed with 4 mol of B to yield 1 mol of C at equilibrium

For the reaction

A(g) + 2B(g)  C(g) + D(g); K_c = 10¹² If the initial moles of A, B, C and D are 0.5, 1, 0.5 and 3.5 moles respectively in a one litre vessel. What is the equilibrium concentration of B ?

The equilibrium constant K_c for the reaction,

A(g) + 2B(g)  3C(g) is 2 × 10^-3

What would be the equilibrium partial pressure of gas C if initial pressure of gas A & B are 1 & 2 atm respectively.

A 20.0 litre vessel initially contains 0.50 mole each of H₂ and I₂ gases. These substances react and finally reach an equilibrium condition. Calculate the equilibrium concentration of HI if K_eq = 49 for the reaction H₂ + I₂  2HI.

A vessel of 250 litre was filled with 0.01 mole of Sb₂S₃ and 0.01 mole of H₂ to attain the equilibrium at 440°c as

Sb₂S₃(s) + 3H₂(g)  2Sb(s) + 3H₂S(g).

After equilibrium the H₂S formed was analysed by dissolving it in water and treating with excess of Pb²⁺ to give. 1.195 g of PbS (Molecular weight = 239) precipitate.

What is value of K_c of the reaction at 440°C ?

The equilibrium constant for the reaction

CO(g) + H₂O(g)  CO₂(g) + H₂(g) is 3 at 500 K. In a 2 litre vessel 60 gm of water gas [equimolar mixture of CO(g) and H₂(g)] and 90 gm of steam is initially taken.

What is the equilibrium concentration of H₂(g) at equilibrium (mole/L) ?

At 87°C, the following equilibrium is established

H₂(g) + S(s)  H₂S(g) K_p = 7 × 10^-2

If 0.50 mole of hydrogen and 1.0 mole of sulfur are heated to 87°C in 1.0 L vessel, what will be the partial pressure of H₂S at equilibrium ?

At certain temperature (T) for the gas phase reaction

2H₂O(g)+2Cl₂(g) 4HCl(g)+O₂(g)       ; K_p =12×10⁸ atm

If Cl₂, HCl & O₂ are mixed in such a manner that the partial pressure of each is 2 atm and the mixture is brought into contact with excess of liquid water. What would be approximate partial pressure of Cl₂ when equilibrium is attained at temperature (T) ?

[Given : Vapour pressure of water is 380 mm Hg at temperature (T)]

At 675 K, H₂(g) and CO₂(g) react to form CO(g) and H₂O(g), K_p for the reaction is 0.16. If a mixture of 0.25 mole of H₂(g) and 0.25 mol of CO₂ is heated at 675 K, mole% of CO(g) in equilibrium mixture is :

In which of the following reactions, increase in the pressure at constant temperature does not affect the moles at equilibrium.

 Change in volume of the system does not alter the number of moles in which of the following equilibrium

The conditions favourable for the reaction :

2SO₂(g)+O₂(g)  2SO₃(g) ; ΔH° = -198 kJ  are :

The exothermic formation of ClF₃ is represented by the equation :

Cl₂(g) + 3F₂(g)  2ClF₃(g)  ;  ΔH = -329 kJ

Which of the following will increase the quantity of ClF₃ in an equilibrium mixture of Cl₂, F₂ and ClF₃ :

Densities of diamond and graphite are 3.5 and 2.3 gm/mL. respectively and for

C(diamond)  C (graphite) ; ΔH= -1.9 kJ/mole favourable conditions for formation of diamond are