At a certain temperature and pressure of 105 Pa, iodine vapour contains 40% by volume of I atoms. The Kp for the equilibrium of the reaction would be-

1. 2.67 $×$ 10Pa

2. 1.00 $×$ 10Pa

3. 3.63 $×$ 10Pa

4. 2.18 $×$ 105 Pa

Subtopic:  Kp, Kc & Factors Affecting them |
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Given the reaction 2HI (g) $⇌$ H2 (g) + I2 (g)

A sample of HI(g) is placed in a flask at a pressure of 0.2 atm. At equilibrium, the partial pressure of HI(g) is 0.04 atm.  The ${\mathrm{K}}_{\mathrm{P}}$ for the given equilibrium would be:

 1 2 2 3.5 3 4 4 2.6
Subtopic:  Kp, Kc & Factors Affecting them |
75%
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A mixture of 1.57 mol of N2, 1.92 mol of H2, and 8.13 mol of NH3 is introduced into a 20 L vessel at 500 K. At this temperature, the equilibrium constant, Kc for the reaction N2 (g) + 3H2 (g) $⇌$ 2NH3 (g) is 1.7 × 102.

The direction of the net reaction is:

1. Reaction is at equilibrium.

2. Reaction will proceed in forwarding direction.

3. Reaction will proceed in the backward direction.

4. Data is not sufficient.

Subtopic:  Kp, Kc & Factors Affecting them |
55%
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Given the reaction:

2BrCl (g) $⇋$ Br2 (g) + Cl2 (g); Kc= 32 at 500 K. If the initial concentration of BrCl is 3.3 × 10-3 mol L–1, the molar concentration of BrCl in the mixture at equilibrium would be:

1. 3.0 $×$ 10-2 molL-1

2. 2.0 $×$ 10-4 molL-1

3. 2.5 $×$ 10-6 molL-1

4. 3.0 $×$ 10-4 molL-1

Subtopic:  Kp, Kc & Factors Affecting them |
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For the reaction, NO(g) + 1/2O2 (g) ⇌ NO2(g)

∆fG° (NO2) = 52.0 kJ/mol , ∆fG° (NO) = 87.0 kJ/mol and
fG° (O2) = 0 kJ/mol.
The equilibrium constant for the formation of NOfrom
NO and O2 at 298K would be

1. 2.36 $×$ 104

2. 3.10 $×$ 107

3. 1.36 $×$ 10${}^{6}$

4. 2.18 $×$ 10${}^{5}$

Subtopic:  Kp, Kc & Factors Affecting them |
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The equilibrium constant for the following reaction is 1.6 ×105 at 1024K

H2(g) + Br2(g)  $⇋$2HBr(g)

If HBr at pressure 10.0 bar is introduced into a sealed container at 1024 K, the equilibrium pressure of HBr will be :

1. 11.20 bar

2. 5.56 bar

3. 7.30 bar

4. 9.95 bar

Subtopic:  Kp, Kc & Factors Affecting them |
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A 0.02 M solution of pyridinium hydrochloride has a pH of 3.44. The ionization constant of pyridine will be:

1. $6.6$ $×$ ${10}^{-6}$

2. $1.51$ $×$ ${10}^{-9}$

3. $2.36$ $×$ ${10}^{-7}$

4. $3.43$ $× {10}^{-9}$

Subtopic:  Salt Hydrolysis & Titration |
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The Ksp of Ag2CrO4 and AgBr is 1.1 × 10–12 and 5.0 × 10–13 respectively.

The molarity ratio of saturated solutions of Ag2CrO4 and AgBr will be:

1. 91.9

2. 108.6

3. 56.9

4. 76.9

Subtopic:  Solubility Product |
51%
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When equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed together (Ksp  (cupric iodate) = 7.4 × 10–8 ), from the following, the correct observation would be :

 1 Precipitation will occur 2 Precipitation will not occur 3 There are 50 % chances of precipitation 4 Data is not sufficient to make any conclusive observation

Subtopic:  Solubility Product |
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The minimum volume of water required to dissolve 1g of calcium sulphate at 298 K is

(For CaSO4Ksp is 9.1 × 10–6)

1. 1.22 L

2. 0.69 L

3. 2.44 L

4. 1.87 L

Subtopic:  Solubility Product |
66%
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