\(\mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{NH}_3\right]^4\left[\mathrm{O}_2\right]^5}{[\mathrm{NO}]^4\left[\mathrm{H}_2 \mathrm{O}]^6\right.}\)
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. | \(\ \mathrm{NH}_{3(\mathrm{g})}+3 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \rightleftharpoons 2 \mathrm{NO}_{(\mathrm{g})}+3 \mathrm{O}_{2(\mathrm{g})}\) |
One 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 |
The equilibrium pressure of C2H6 when it is placed in a flask at 4.0 atm pressure at 899 K would be:
C2H6 (g) C2H4 (g) + H2 (g)
(Kp = 0.04 atm at 899 K)
1. | 4.12 atm | 2. | 3.62 atm |
3. | 1.54 atm | 4. | 2.16 atm |
A sample of pure PCl5 was introduced into an evacuated vessel at 473 K.
After equilibrium was attained, a concentration of PCl5
was found to be 0.5 × 10–1 mol L–1. If the value of
Kc is 8.3 × 10–3 mol L–1, the concentrations of
PCl3 and Cl2 at equilibrium would be:
PCl5 (g) PCl3 (g) + Cl2(g)
1. | |
2. | |
3. | |
4. |
Match the following equilibria with the corresponding condition.
A. | LiquidVapour | 1. | Saturated solution |
B. | SolidLiquid | 2. | Boiling point |
C. | SolidVapour | 3. | Sublimation point |
D. | Solute (s)Solute (solution) | 4. | Melting point |
5. | Unsaturated solution |
Codes:
A | B | C | D | |
1. | 2 | 4 | 3 | 1 |
2. | 1 | 2 | 3 | 5 |
3. | 5 | 4 | 3 | 2 |
4. | 4 | 5 | 3 | 2 |
Column I (Reaction) | Column II (Equilibrium constant) |
A. | 1. |
B. | 2. |
C. | 3. |
4. |
Codes:
A | B | C | |
1. | 4 | 3 | 2 |
2. | 1 | 2 | 3 |
3. | 1 | 4 | 3 |
4. | 4 | 1 | 3 |
Match the standard free energy of the reaction with the corresponding equilibrium constant.
A. | 1. K>1 |
B. | 2. K=1 |
C. | 3. K=0 |
4. K<1 |
Codes:
A | B | C | |
1. | 4 | 1 | 2 |
2. | 1 | 2 | 3 |
3. | 2 | 4 | 3 |
4. | 4 | 1 | 3 |
Match the following species with the corresponding conjugate acid:
Species | Conjugate acid |
A. | 1. |
B. | 2. |
C. | 3. |
D. | 4. |
5. |
Codes
A | B | C | D | |
1. | 2 | 5 | 1 | 5 |
2. | 2 | 4 | 3 | 5 |
3. | 5 | 4 | 3 | 2 |
4. | 4 | 5 | 3 | 2 |
Given below are two statements:
Assertion (A): | The increasing order or acidity of hydrogen halides is HF<HCI<HBr<HI. |
Reason (R): | While comparing acids formed by the elements belonging to the same group of the periodic table, H-A bond strength is a more important factor in determining the acidity of an acid than the polar nature of the bond. |
1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
3. | (A) is True but (R) is False. |
4. | (A) is False but (R) is True. |
Given below are two statements:
Assertion (A): | A solution containing a mixture of acetic acid and sodium acetate maintains a constant value of pH on the addition of small amounts of acid or alkali. |
Reason (R): | A solution containing a mixture of acetic acid and sodium acetate acts as a buffer solution. |
1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
3. | (A) is True but (R) is False. |
4. | (A) is False but (R) is True. |