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Q. No.The reaction, among the following, that has ∆S° > 0 is:
1.
S8(l) → S8(s, monoclinic)
2.
H2(g) + O2(g) → H2O2(aq)
3.
H2(g) + 2 Ag+(aq) → 2 H+(aq) + 2 Ag(s)
4.
PCl5(g) → PCl3(g) + Cl2(g)
Subtopic: Spontaneity & Entropy |
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Given below are two statements:
| Assertion (A): | Variables like P, V, and T are called state functions. |
| Reason (R): |
Their values depend solely on the system's state, and not on how it is reached. |
| 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. | Both (A) and (R) are False. |
Subtopic: Thermodynamics' Properties and process |
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At 1 atm pressure,
\(\mathrm{\Delta S = 75 \ JK^{-1} mol^{-1} \ and \ \Delta H = 30 \ kJ mol^{-1} }\).
The temperature at which the reaction attains equilibrium is:
\(\mathrm{\Delta S = 75 \ JK^{-1} mol^{-1} \ and \ \Delta H = 30 \ kJ mol^{-1} }\).
The temperature at which the reaction attains equilibrium is:
| 1. | 400 K | 2. | 330 K |
| 3. | 200 K | 4. | 110 K |
Subtopic: Spontaneity & Entropy |
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Given the following reaction:
\(\mathrm{Ag}_2 \mathrm{O}(s) \rightarrow 2 \mathrm{Ag}(s)+\frac{1}{2} \mathrm{O}_2(g)\)
The values of \(\Delta H\) and \(\Delta S\) are 30.56 kJ/mol and 66.00 J/Kmol, respectively.
The temperature at which the free energy change (\(\Delta G\)) for the reaction will be zero is:
1. 563 K
2. 463 K
3. 403 K
4. 544 K
\(\mathrm{Ag}_2 \mathrm{O}(s) \rightarrow 2 \mathrm{Ag}(s)+\frac{1}{2} \mathrm{O}_2(g)\)
The values of \(\Delta H\) and \(\Delta S\) are 30.56 kJ/mol and 66.00 J/Kmol, respectively.
The temperature at which the free energy change (\(\Delta G\)) for the reaction will be zero is:
1. 563 K
2. 463 K
3. 403 K
4. 544 K
Subtopic: Gibbs Energy Change |
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A sample of 54.0g of methanol is heated from 25.0°C to 35.0°C. The amount of heat required is: (Given: The specific heat capacity of methanol is 2.48 J g–1 K–1)
| 1. | 0.00459 J | 2. | 0.0747 J |
| 3. | 1340 J | 4. | 4690 J |
Subtopic: Enthalpy & Internal energy |
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At which of the following conditions does a reaction with positive \(\Delta \mathrm{H} \) becomes spontaneous?
1. \(\Delta S=+ve \) , low temperature
2. \(\Delta S=+ve, \) high temperature
3. \(\Delta S=-ve,\) at all temperature
4. \(\Delta S=- \text {ve}\), at low temperature
1. \(\Delta S=+ve \) , low temperature
2. \(\Delta S=+ve, \) high temperature
3. \(\Delta S=-ve,\) at all temperature
4. \(\Delta S=- \text {ve}\), at low temperature
Subtopic: Spontaneity & Entropy |
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Match Column I (Reactions) with Column II (Enthalpy) and mark the appropriate choice:
1. (A) →(iv), (B)→(iii), (C) →(i), (D)→ (ii)
2. (A) →(ii), (B)→(i), (C) →(iv), (D)→ (iii)
3. (A) →(i), (B)→(ii), (C) →(iii), (D)→ (iv)
4. (A) →(iii), (B)→(iv), (C) →(ii), (D)→ (i)
| Column I (Reactions) | Column II (Enthalpy) | ||
| (A) | \(\small{CH_{4(g)} + 2O_{2(g)} \rightarrow CO_{2(g)} + 2H_2O}\) | (i) | \(\Delta _{sol}H^o\) |
| (B) | \( H_{2(g)} \rightarrow 2H_{(g)}\) | (ii) | \(\Delta _{lattice}H^o\) |
| (C) | \(NaCl_{(s)} \rightarrow Na^+_{(g)} + Cl^-_{(g)} \) | (iii) | \(\Delta _{c}H^o\) |
| (D) | \(NaCl_{(s)} \rightarrow Na^+_{(aq)} + Cl^-_{(aq)} \) | (iv) | \(\Delta _{bond}H^o\) |
1. (A) →(iv), (B)→(iii), (C) →(i), (D)→ (ii)
2. (A) →(ii), (B)→(i), (C) →(iv), (D)→ (iii)
3. (A) →(i), (B)→(ii), (C) →(iii), (D)→ (iv)
4. (A) →(iii), (B)→(iv), (C) →(ii), (D)→ (i)
Subtopic: Thermochemistry |
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What is the enthalpy change (ΔH) for the reaction represented by the equation, \(\mathrm{OF_2 + H_2O \rightarrow O_2+2HF?}\)
[Given the bond energies of \(\mathrm{O-F, O-H, H-F}\) \(\mathrm {and~O=O}\) as 44, 111, 135, and 119 kcal mol–1, respectively]
[Given the bond energies of \(\mathrm{O-F, O-H, H-F}\) \(\mathrm {and~O=O}\) as 44, 111, 135, and 119 kcal mol–1, respectively]
| 1. | –222 kcal | 2. | –88 kcal |
| 3. | –111 kcal | 4. | –79 kcal |
Subtopic: Thermochemistry |
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Match Column-I with Column-II and mark the appropriate choice:
1. (A) →(iii), (B)→(i), (C) →(iv), (D)→ (ii)
2. (A) →(ii), (B)→(iv), (C) →(i), (D)→ (iii)
3. (A) →(ii), (B)→(iv), (C) →(iii), (D)→ (i)
4. (A) →(iii), (B)→(ii), (C) →(i), (D)→ (iv)
| Column-I | Column-II | ||
| (A) | State Function | (i) | At constant pressure |
| (B) | \(\Delta H = q\) | (ii) | Specific heat |
| (C) | \(\Delta U = q\) | (iii) | Entropy |
| (D) | Intensive property | (iv) | At constant volume |
1. (A) →(iii), (B)→(i), (C) →(iv), (D)→ (ii)
2. (A) →(ii), (B)→(iv), (C) →(i), (D)→ (iii)
3. (A) →(ii), (B)→(iv), (C) →(iii), (D)→ (i)
4. (A) →(iii), (B)→(ii), (C) →(i), (D)→ (iv)
Subtopic: Enthalpy & Internal energy | Classification of System, Extensive & Intensive Properties |
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The temperature at which the given reaction is in equilibrium is:
\(\mathrm{X_{(g)} +3Y_{(g)} \rightleftharpoons 2Z_{(g)} ; \Delta H= -40~ kJ ~mol^{-1}}~\)
(The standard entropies of X, Y, and Z are 60, 40, and 50 J K–1 mol–1, respectively.)
1. 273 K
2. 600 K
3. 500 K
4. 400 K
\(\mathrm{X_{(g)} +3Y_{(g)} \rightleftharpoons 2Z_{(g)} ; \Delta H= -40~ kJ ~mol^{-1}}~\)
(The standard entropies of X, Y, and Z are 60, 40, and 50 J K–1 mol–1, respectively.)
1. 273 K
2. 600 K
3. 500 K
4. 400 K
Subtopic: 2nd & 3rd Law of Thermodynamics |
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