JEE Advanced (One or More Correct Option): Equilibrium | Chapter-wise Tests for JEE Main & Advanced PDF Download

Q.1.

The correct relations among the following are
(a) K₁x K₃= 1
(b)
(c)
(d)

Correct Answer is option (a, b and c)

Q.2. Consider the reaction 
2CO (g) + O₂ (g) ⇌ 2CO₂ (g) + Heat

Under what conditions shift is undeterminable?
(a) Addition of O₂ and decrease in volume
(b) Addition of CO and removal of CO₂ at constant volume
(c) Increase in temperature and decrease in volume
(d) Addition of CO and increase in temperature at constant volume

Correct Answer is option (c, d)
Le Chatelier’s principle is not quantitative. If both stress would cause the same direction of shift, the shift is determinable. If the two stresses would cause shifts in opposite directions, no deduction is possible.

Q.3. For the reaction PCl₅ (g) ⇌ PCl₃ (g) + Cl₂(g), the forward reaction at constant temperature is favoured by -
(a) introducing an inert gas at constant volume
(b) introducing chlorine gas at constant volume
(c) introducing an inert gas at constant pressure
(d) increasing the volume of the container

Correct Answer is option (c, d)
Moles at equilibrium

If total pressure at equilibrium is P_T

On adding inert gas at constant pressure volume increases and thus

Q.4. The rate law for the decomposition of NH₃; i.e.
2NH₃ → N₂ + 3H₂; is given by  

which one of the following is/are incorrect for it.

(a) When the concentration of NH3 is very high; order lies between zero and one.
(b) When the concentration of NH3 is very high; order is zero
(c) When the concentration of NH3 is very low; order is zero.
(d) When the concentration of NH3 is very low; order is two.

Correct Answer is option (a, c and d)

If [NH₃] is very high  is very small than k<sub>2

i.e. order is zero
If [NH3] is very low  is very high than k2</sub>

∴ order is one.

Q.5.

Following the graph, which of the statement/s is/are correct?
(a) The absolute conversion of N₂O₄ into NO₂(N₂O₄ →2NO₂) is spontaneous
(b) The dynamic conversion (N₂O₄⇔2NO₂) at equilibrium point is spontaneous
(c) Formation of N₂O₄ is more spontaneous than dissociation
(d) Both process dissociation as well as formation are equally spontaneous.

Correct Answer is option (b, c)
As  (positive) that’s why direct conversion I non-spontaneous. But at equilibrium point BN₂O₄ is dissociated upto equilibrium point (dissociation of that extent) spontaneous as ΔG° =-0.86kJ

Hence, dynamic conversion N₂O₄ upto equilibrium point is fairly spontaneous

Hence, dynamic conversion N2O4 into equilibrium mixture and 2NO₄ into equilibrium mixture both are spontaneous But, as for the reverse process ΔG° is – 6.24 kJ (more than forward), that’s why more favourable.

Q.6. 100 ml of 0.5 M CH3COOH is dissolved is 200 ml of M/4
NaOH solution; which of the following statement is correct? (Given K_a = 10^–5)
(a) Buffer solution will be formed
(b) Anionic hydrolysis will occur
(c) pH of resultant solution will be > 7 at 25°C
(d) Solution will be Neutral so pH = 7

Correct Answer is option (b, c)

Q.7. pH of saturated aqueous solution of Ba(OH)₂ is 12. Identify the correct statement.

(a) The solubility of Ba(OH)₂ in a buffer solution of pH=13 is 5x 10^–5 moles/L

(b) The solubility of Ba(OH)₂ decreases in presence of NH4Cl

(c) The solubility of Ba(OH)₂ in a buffer solution of pH=1 is 5 x 10^–5 moles/L

(d) The solubility product of Ba(OH)₂ is 5 x 10^–7M³

Correct Answer is option (a, d)

Q.8. In which of the following solvent the solubility of AgCl is more than solubility of AgCl in cold water

(a) NaCl Solution

(b) solution of NH₃

(c) AgNO₃ solution

(d) Hot water

Correct Answer is option (b, d)

Ag⁺ ion combine with NH₃ to form complex compound (Ag(NH₃)₂ ]²⁺ hence solubility of increase solubility of increase with temperature.

Q.9. 10 mL of a weak acid (HA) is 20% dissociated in water. The solution is completely neutralized by 10mL of  2 x10^-3 M  NaOH solution. Which of the following are true?

(a) pH of the weak acid is 3.4

(b) K_a of the weak acid is 10^-4

(c) pH of the solution at the equivalence point is 7.5

(d) K_h of aq NaA is 10^-9

Correct Answer is option (a, b and c)

pH at equivalence point = 7.5

Q.10. Identify the correct statement.
(a) H₂O can act as Arrhenius acid, Lowry–Bronsted acid as well as Lewis acid

(b) At 25°C pK_a of H₂O is 15.75 and pK_b is -1.75

(c) % dissociation of water at 25°C is 1.8 x 10^-7

(d) pK_a of H₃O⁺ ion is –1.75 at 25°C (log 1.8 = 0.25)

Correct Answer is option (c, d)

(b) pK_a and pK_b of H₂O are same 15.75
(c) % dissociation
(d) H₂O can not act as Lewis acid.