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. 2.67 104 Pa
2. 1.00 105 Pa
3. 3.63 104 Pa
4. 2.18 105 Pa
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NEET MCQ Books for XIth & XIIth Physics, Chemistry & BiologyGiven 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 for the given equilibrium would be:
1. | 2.0 | 2. | 3.5 |
3. | 4.0 | 4. | 2.6 |
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NEET MCQ Books for XIth & XIIth Physics, Chemistry & BiologyA 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.
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NEET MCQ Books for XIth & XIIth Physics, Chemistry & BiologyGiven 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
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NEET MCQ Books for XIth & XIIth Physics, Chemistry & BiologyFor 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 NO2 from NO and O2 at 298K would be:
1. | 2.36 104 | 2. | 3.10 107 |
3. | 1.36 10 | 4. | 2.18 10 |
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NEET MCQ Books for XIth & XIIth Physics, Chemistry & BiologyThe 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
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NEET MCQ Books for XIth & XIIth Physics, Chemistry & BiologyFor the reaction, 2NOCl (g) 2NO (g) + Cl2 (g); Kp= 1.8 × 10–2 atm at 500 K.
The value of Kc for above mentioned reaction would be:
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NEET MCQ Books for XIth & XIIth Physics, Chemistry & BiologyFor the following equilibrium, Kc= 6.3 × 1014 at 1000 K
The value of Kc for the reverse reaction is:
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NEET MCQ Books for XIth & XIIth Physics, Chemistry & Biology\(\mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{NH}_3\right]^4\left[\mathrm{O}_2\right]^5}{[\mathrm{NO}]^4\left[\mathrm{H}_2 \mathrm{O}]^6\right.}\)
The balanced chemical equation corresponding to the above-mentioned expression is:
1. | \(4 \mathrm{NO}_{(\mathrm{g})}+6 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \rightleftharpoons 4 \mathrm{NH}_{3(\mathrm{g})}+5 \mathrm{O}_{2(\mathrm{g})} \) |
2. | \(4 \mathrm{NH}_3(\mathrm{g})+5 \mathrm{O}_{2(\mathrm{g})} \rightleftharpoons 4 \mathrm{NO}_{(\mathrm{g})}+6 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}\) |
3. | \(\ 2 \mathrm{NO}_{(\mathrm{g})}+3 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \rightleftharpoons 4 \mathrm{NH}_{3(\mathrm{g})}+3 \mathrm{O}_{2(\mathrm{g})}\) |
4. | \(\ \mathrm{NH}_{3(\mathrm{g})}+3 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \rightleftharpoons 2 \mathrm{NO}_{(\mathrm{g})}+3 \mathrm{O}_{2(\mathrm{g})}\) |
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NEET MCQ Books for XIth & XIIth Physics, Chemistry & BiologyOne mole of H2O and one mole of CO are taken in a 10 L vessel and heated to 725 K. At equilibrium, 40% of water(by mass) reacts with CO according to the equation,
H2O (g) + CO (g) H2 (g) + CO2 (g)
The equilibrium constant for the above-mentioned reaction would be:
1. | 0.66 | 2. | 0.35 |
3. | 0.44 | 4. | 0.82 |
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NEET MCQ Books for XIth & XIIth Physics, Chemistry & Biology