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Q. No.For the reaction,
\(N_2(g) + 3H_2 (g) \rightleftharpoons 2NH_3(g) \), on adding inert gas at constant volume, equilibrium:
1.
shifts in the forward reaction
2.
shifts in backward reaction
3.
remains unaffected
4.
Initially in the forward direction and then in the backward direction
Subtopic: Le Chatelier's principle |
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For the reaction,
\(H_2NCOONH_4 (s) \rightleftharpoons2 NH_3(g) + CO_2(g)\), the total pressure at equilibrium is 15 atmospheres. It can be concluded that the value of \(K_P\) will be:
1. 15 atm3
2. 50 atm3
3. 500 atm3
4. 100 atm3
\(H_2NCOONH_4 (s) \rightleftharpoons2 NH_3(g) + CO_2(g)\), the total pressure at equilibrium is 15 atmospheres. It can be concluded that the value of \(K_P\) will be:
1. 15 atm3
2. 50 atm3
3. 500 atm3
4. 100 atm3
Subtopic: Kp, Kc & Factors Affecting them |
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Given below are two statements:
| Assertion (A): | If Qp<Kp reaction moves in the direction of reactants. |
| Reason (R): | The reaction quotient is defined in the same way as the equilibrium constant at any stage of the reaction. |
| 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. |
Subtopic: Introduction To Equilibrium |
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Initially 2 moles of \(NOCl \) taken in 1 L of closed container and it dissociates into NO and Cl2 gas.
The reaction is as follows:
\(2 \mathrm{NOCl}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Cl}_2(g)\)
Calculate the equilibrium constant Kc given that 0.4 moles of NO is obtained at equilibrium.
The reaction is as follows:
\(2 \mathrm{NOCl}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Cl}_2(g)\)
Calculate the equilibrium constant Kc given that 0.4 moles of NO is obtained at equilibrium.
| 1. | 142 × 10-4 | 2. | 142 × 10-6 |
| 3. | 125 × 10-4 | 4. | 130 × 104 |
Subtopic: Introduction To Equilibrium |
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A weak acid is titrated with a weak base. Consider the following statements regarding the pH of the solution at the equivalence point:
The correct statements are :
| (i) | pH depends on the concentration of acid and base. |
| (ii) | pH is independent of the concentration of acid and base. |
| (iii) | pH depends on pKa of acid and pKb of base. |
| (iv) | pH is independent of pKa of acid and pKb of base. |
| 1. | only (i) and (iii) | 2. | only (i) and (iv) |
| 3. | only (ii) and (iii) | 4. | only (ii) and (iv) |
Subtopic: pH calculation |
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If 0.01 M acetic acid solution is 1% ionised, then pH of this acetic acid solution is:
| 1. | 3 | 2. | 2 |
| 3. | 4 | 4. | 1 |
Subtopic: pH calculation |
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NEET 2025 - Target Batch
The solubility of BaSO4 in 10-3 M H2SO 4 solution will be:
(Given: Ksp for BaSO4 = 1.1 × 10-10)
(Given: Ksp for BaSO4 = 1.1 × 10-10)
| 1. | 1.1 × 10–13 M | 2. | 1.1 × 10–7 M |
| 3. | 5.5 × 10–7 M | 4. | 5.5 × 10–8 M |
Subtopic: Solubility Product |
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The solubility of \(Sr(OH)_2 \) at 298 K is 20 g/L of solution. The pH of this solution will be:
(Given: molar mass of Sr = 88 g/mol; log 40 =1.60 ; and log 122 = 2.086)
1. 13.51
2. 0.48
3. 10.22
4. 11.25
(Given: molar mass of Sr = 88 g/mol; log 40 =1.60 ; and log 122 = 2.086)
1. 13.51
2. 0.48
3. 10.22
4. 11.25
Subtopic: Solubility Product |
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Select the correct order of solubility of AgCl in the following solutions:
(a) \(0.1 \text {M NaCl (aq)} \)
(b) \(0.1~ \text {M} ~\text {CaCl}_2 ~ (\text {aq}) \)
(c) \(0.1~ \text {M} ~\text {AlCl}_3 ~ (\text {aq}) \)
1. (a) = (b) = (c)
2. (a) > (b) > (c)
3. (a) < (b) < (c)
4. (c) > (b) = (a)
(a) \(0.1 \text {M NaCl (aq)} \)
(b) \(0.1~ \text {M} ~\text {CaCl}_2 ~ (\text {aq}) \)
(c) \(0.1~ \text {M} ~\text {AlCl}_3 ~ (\text {aq}) \)
1. (a) = (b) = (c)
2. (a) > (b) > (c)
3. (a) < (b) < (c)
4. (c) > (b) = (a)
Subtopic: Common Ion Effect |
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100 ml of \(HCl\) (pH=1) is mixed with 150 ml of \(HCl\) (pH =2). The pH of the resulting solution will be:
(log 4.6 = 0.65)
1. 1.35
2. 1.5
3. 1.8
4. 1.9
(log 4.6 = 0.65)
1. 1.35
2. 1.5
3. 1.8
4. 1.9
Subtopic: pH calculation |
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