Q. No.\(\mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{NH}_3\right]^4\left[\mathrm{O}_2\right]^5}{[\mathrm{NO}]^4\left[\mathrm{H}_2 \mathrm{O}]^6\right.}\)
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.
\(\ \mathrm{NH}_{3(\mathrm{g})}+3 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \rightleftharpoons 2 \mathrm{NO}_{(\mathrm{g})}+3 \mathrm{O}_{2(\mathrm{g})}\)
The balanced chemical equation corresponding to the above-mentioned expression is:
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. | Liquid ⇌ Vapour | I. | Saturated solution |
| B. | Solid ⇌ Liquid | II. | Boiling point |
| C. | Solid ⇌ Vapour | III. | Sublimation point |
| D. | Solute (s) ⇌ Solute (solution) | IV. | Melting point |
| V | Unsaturated solution |
Codes:
| A | B | C | D | |
| 1. | II | IV | III | I |
| 2. | I | II | III | V |
| 3. | V | IV | III | II |
| 4. | IV | V | III | II |
Match the following reactions with the corresponding equilibrium constant:
| Column-I (Reaction) | Column-II (Equilibrium constant) | ||
| A. | (i) | ||
| B. | (ii) | ||
| C. | (iii) | ||
| (iv) |
(Given that reference, Kc is the equilibrium constant for the ammonia synthesis.)
Codes:
| A | B | C | |
| 1. | (iv) | (iii) | (ii) |
| 2. | (i) | (ii) | (iii) |
| 3. | (i) | (iv) | (iii) |
| 4. | (iv) | (i) | (iii) |
Match the standard free energy of the reaction with the corresponding equilibrium constant:
| A | \(\Delta \mathrm{G}^{\ominus}>0\) | (a) | K>1 |
| B | \(\Delta \mathrm{G}^{\ominus}<0\) | (b) | K=1 |
| C | \(\Delta \mathrm{G}^{\ominus}=0\) | (c) | K=0 |
| (d) | K<1 |
Codes:
| A | B | C | |
| 1. | (d) | (a) | (b) |
| 2. | (a) | (b) | (c) |
| 3. | (b) | (d) | (c) |
| 4. | (d) | (a) | (c) |
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. |
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