1. A mixture of H_{2} and I_{2} in molecular proportion of 2 : 3 was heated at 444°C till the reaction H_{2} + I_{2} ⇌ 2HI reached equilibrium state. Calculate the percentage of iodine converted into HI. (K_{C} at 444°C is 0.02)

a) 4.38%

b) 6.38%

c) 5.38%

d) 3.38%

Explanation:

2. 2SO_{2}(g) + O_{2}(g) ⇌ 2SO_{3} (g)

If the partial pressure of SO_{2}, O_{2} and SO_{3} are 0.559, 0.101 and 0.331 atm respectively. What would be the partial pressure of O_{2} gas, to get equal moles of SO_{2} and SO_{3}.

a) 0.288 atm

b) 0.388 atm

c) 0.488 atm

d) 0.188 atm

Explanation:

3. The equilibrium constant of the reaction A_{2} (g) + B_{2}(g) ⇌ 2AB (g) at 100°C is 50. If one litre flask containing one mole of A_{2} is connected to a 3 litre flask containing two moles of B_{2} the number of moles of AB formed at 373 K will be -

a) 0.943

b) 18.86

c) 2.317

d) 1.886

Explanation:

4. The equilibrium constant K, for the reaction N_{2} + 3H_{2} ⇌ 2NH_{3} is 1.64 × 10^{-4} atm^{-2} at 300°C. What will be the equilibrium constant at 400°C, if heat of reaction in this temperature range is – 105185.8 Joules.

a) 0.64 × 10^{-5} atm^{-2}

b) 6.4 × 10^{-3} atm^{-2}

c) 0.64 × 10^{-3} atm^{-2}

d) 0.64 × 10^{-1} atm^{-2}

Explanation:

5. When 1.0 mole of N_{2} and 3.0 moles of H_{2} was heated in a vessel at 873 K and a pressure of 3.55 atm. 30% of N_{2} is converted into NH_{3} at equilibrium. Find the value of K_{P} for the reaction.

a) 4.1 × 10^{-2} atm^{-2}

b) 5.1 × 10^{-2} atm^{-2}

c) 6.1 × 10^{-2} atm^{-2}

d) 3.1 × 10^{-2} atm^{-2}

Explanation:

6. A_{2}(g) and B_{2}(g) at initial partial pressure of 98.4 and 41.3 torr, respectively were allowed to react at 400 K. At equilibrium the total pressure was 110.5 torr. Calculate the value of K_{P} for the following reaction at 400 K.

2A_{2}(g) + B_{2}(g) ⇌ 2 A_{2}B (g)

a) 134

b) 154

c) 124

d) 174

Explanation:

7. Ammonium hydrogen sulphide dissociated according to the equation,
NH_{4}HS (s) ⇌ NH_{3}(g) + H_{2}S (g). If the observed pressure of the mixture is 2.24 atm at 106°C, what is the equilibrium constant K_{p} of the reaction ?

a) 3.2764 atm^{2}

b) 1.2544 atm^{2}

c) 2.3247 atm^{2}

d) 8.1267 atm^{2}

Explanation:

8. For the reaction, CaCO_{3}(s) ⇌ CaO(s) + CO_{2} (g) ; K = 0.059 atm at 1000 K. 1 g of CaCO_{3} is placed in a 10 litre container at 1000 K to reach the equilibrium. Calculate the mass of CaCO_{3} left at equilibrium.

a) 0.38 g

b) 0.18 g

c) 0.28 g

d) 0.72 g

Explanation:

9. In a mixture of N_{2} and H_{2}, initially they are in a mole ratio of 1 : 3 at 30 atm and 300°C, the percentage of ammonia by volume under the equilibrium is 17.8%. Calculate the equilibrium constant (K_{p}) of the mixture, for the reaction, N_{2}(g) + 3H_{2}(g) ⇌ 2NH_{3}(g).

a) 3.61 × 10^{-4} atm^{-2}

b) 5.47 × 10^{-4} atm^{-2}

c) 2.24 × 10^{-4} atm^{-2}

d) 7.31 × 10^{-4} atm^{-2}

Explanation:

10. Given below are the values of ∆H° and ∆S° for the reaction at 27°C,

SO_{2}(g) + 1/2 O_{2}(g) ⇌ SO_{3}(g)

∆H° = 98.32 kJ/mol

∆S° = –95 J/mol. Calculate the value of K_{p}
for the reaction.

a) 1.44 × 10^{12} atm^{-1/2}

b) 2.39 × 10^{12} atm^{-1/2}

c) 7.52 × 10^{12} atm^{-1/2}

d) 4.61 × 10^{12} atm^{-1/2}

Explanation: