PrepBharat

1. A mixture of H₂ and I₂ in molecular proportion of 2 : 3 was heated at 444°C till the reaction H₂ + I₂ ⇌ 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%

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2. 2SO₂(g) + O₂(g) ⇌ 2SO₃ (g)
If the partial pressure of SO₂, O₂ and SO₃ are 0.559, 0.101 and 0.331 atm respectively. What would be the partial pressure of O₂ gas, to get equal moles of SO₂ and SO₃.
a) 0.288 atm
b) 0.388 atm
c) 0.488 atm
d) 0.188 atm

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3. The equilibrium constant of the reaction A₂ (g) + B₂(g) ⇌ 2AB (g) at 100°C is 50. If one litre flask containing one mole of A₂ is connected to a 3 litre flask containing two moles of B₂ the number of moles of AB formed at 373 K will be -
a) 0.943
b) 18.86
c) 2.317
d) 1.886

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4. The equilibrium constant K, for the reaction N₂ + 3H₂ ⇌ 2NH₃ 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

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5. When 1.0 mole of N₂ and 3.0 moles of H₂ was heated in a vessel at 873 K and a pressure of 3.55 atm. 30% of N₂ is converted into NH₃ 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

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6. A₂(g) and B₂(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.
2A₂(g) + B₂(g) ⇌ 2 A₂B (g)
a) 134
b) 154
c) 124
d) 174

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7. Ammonium hydrogen sulphide dissociated according to the equation, NH₄HS (s) ⇌ NH₃(g) + H₂S (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 atm²
b) 1.2544 atm²
c) 2.3247 atm²
d) 8.1267 atm²

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8. For the reaction, CaCO₃(s) ⇌ CaO(s) + CO₂ (g) ; K = 0.059 atm at 1000 K. 1 g of CaCO₃ is placed in a 10 litre container at 1000 K to reach the equilibrium. Calculate the mass of CaCO₃ left at equilibrium.
a) 0.38 g
b) 0.18 g
c) 0.28 g
d) 0.72 g

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9. In a mixture of N₂ and H₂, 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, N₂(g) + 3H₂(g) ⇌ 2NH₃(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

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10. Given below are the values of ∆H° and ∆S° for the reaction at 27°C,
SO₂(g) + 1/2 O₂(g) ⇌ SO₃(g)
∆H° = 98.32 kJ/mol
∆S° = –95 J/mol. Calculate the value of K_p for the reaction.
a) 1.44 × 10¹² atm^-1/2
b) 2.39 × 10¹² atm^-1/2
c) 7.52 × 10¹² atm^-1/2
d) 4.61 × 10¹² atm^-1/2

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