Equilibrium Test (18-12-2016) - IIT JAM MCQ

For the reaction, if percentage dissociation of N₂O₄ are 25%, 50%, 75% and 100%, then the sequence of observed vapour densities will be:

For the reaction, if the initial concentration of [H₂] = [CO₂] and x mol/litre of H₂ is consumed at equilibrium, the correct expression of K_p is:

H₃PO₄ is a tribasic acid, it undergoes ionization as:

Then, equilibrium constant for the followimg reaction will be:

The equilibrium constant for the reaction is 5. How many moles of CO₂ must be added to 1 litre container already containing 3 moles each of CO and H₂O to make 2M equilibrium concentration of CO?

A nitrogen–hydrogen mixture initially in the molar ratio of 1:3 reacted equilibrium to form ammonia when 25% of the N₂ and H₂ had reached. If the total pressure of the system was 21 atm, the partial pressure of ammonia at the equilibrium was:

The freezing point depression constant for water is 1.86°C m^–1. If 5 g Na₂SO₄ is dissolved in 45 g H₂O, the freezing point is changed by –3.82°C. Calculate the van't Hoff factor for Na₂SO_4. 

K_sp(AgCl) > K_sp(AgBr) > K_sp(AgI). This means that:

The triple point for water is:

At 25°C, the volue of Pk_b (K_b being the dissociation constant as a base) for NH₃ in aqueous solution is 4.7. What is the pH of 0.1 M aqueous solution of NH₄Cl with 0.01 M NH₃ (approxmately):

The solution of CaF₂(K_sp = 3.4 × 10^–11) in 0.1 M solution of NaF would be:

For the chemical equilibrium can be determined from which one of the following plots?

On adding 0.1 M solution each of Ag⁺, Ba²⁺ and Ca²⁺ in an Na₂SO₄ solution, the species first precipitated is (K_sp BaSO₄ = 10^–11, K_sp CaSO₄ = 10^–6, K_sp Ag₂SO₄ = 10^–5):

Which of the following expression for % ionization of a mono-acidic base (BOH) in aqueous solution at appreciable concentration is correct?

Which of the Following is/are affected by pressure change?

A buffer solution can be prepared from a mixture of?

The equilibrium in aqueous medium at 25⁰C shifts towards the left in the presence of:

Choose the correct statements:

The solubility of Pb(OH)₂ in water is 6.7x10^-6M. The solubility of Pb(OH)₂ in a buffer solution of PH=8 is 1.2x10^-x what is the value of x

3.1 mole of FeCl₃ and 3.2 mole of NH₄SCN are added tone litre of water. At equilibrium, 3.0 mol of FeSCN²⁺ are formed. The equilibrium constant Kc of the reaction,

 will be:

The equilibrium of formation of phosgene is represented as:

The reaction is carried out in a 500 ml flask. At equilibrium 0.3 mole of phosgene, 0.1 mole of CO and 0.1 mole of Cl₂ are present. The equilibrium constant of the reaction is:

SO_3(g) is heated in a closed vessel. An equilibrium:  is established. The vapour density of the mixture, in which SO₃ is 50% dissociated, is:

The dissociation constant of a substituted benzoic acid at 25⁰C is 1.0x10^-4. The PH of 0.01M solution of its sodium salt is.

Consider the following reversible system:

At equilibrium, there are 1.0 mole of A and 2.0 moles of each B,C & D present. If 2.0 mole of B is added further, how many moles of C would be required to be added so that mole of A & D do not change?

0.10 mole each of SO₂ and SO₃ are mixed in a 2.0 dm³ flask at 300K. Equilibrium is attained as  

equilibrium pressure is 281.68 kpa. The mole fraction of O₂

In the Reaction,  if D and d are the vapour densities at initial stage and at equilibrium then what will be the value of  at point A in the following graph?

The number of degree of freedom of a system consisting of solid sucrose in equilibrium with an aqueous solution of sucrose is:

0.16 g of N₂H₄ are dissolved in water and the total volume made up to 500 mL. Calculate the percentage of N₂H₄ that has reacted with water at this dilution. The K_b for N₂H₄ is 4.0 × 10^–6 M: