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Q. No.Match the process name given in Column-I with the corresponding data in Column-II and mark the appropriate option.
Column-I
Column-II
(A)
Exothermic
(i)
\(\Delta H= 0 , \Delta U =0\)
(B)
Spontaneous
(ii)
\(\Delta G=0~\)
(C)
Cyclic process
(iii)
\(\Delta H\) is negative
(D)
Equilibrium
(iv)
\(\Delta G\) is negative
1. (A) →(ii), (B)→(iii), (C) →(i), (D)→ (iv)
2. (A) →(iv), (B)→(i), (C) →(iii), (D)→ (ii)
3. (A) →(i), (B)→(ii), (C) →(iv), (D)→ (iii)
4. (A) →(iii), (B)→(iv), (C) →(i), (D)→ (ii)
Subtopic: Thermodynamics' Properties and process | Spontaneity & Entropy |
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Five moles of an ideal gas at 1 bar and 298 K undergo free expansion (expansion into vacuum) such that its volume becomes double. Calculate the work done during the process:
2. \( \text {-RT }\left(\mathrm{V}_2-\mathrm{V}_1\right) \)
3. \( \text {-RT } \ln \mathrm({V}_1 / \mathrm{V}_2 )\)
4. Zero
Subtopic: First Law of Thermodynamics | Enthalpy & Internal energy |
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Identify the intensive quantities/properties from the following:
1. (a), (b) and (c)
2. (b) and (d)
3. (d) and (a)
4. None of the above
| (a) | Enthalpy | (b) | Temperature |
| (c) | Volume | (d) | Refractive Index |
1. (a), (b) and (c)
2. (b) and (d)
3. (d) and (a)
4. None of the above
Subtopic: Classification of System, Extensive & Intensive Properties |
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Level 2: 60%+
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Consider the data in the table given below and choose the correct answer:
The molar enthalpy of vapourisation of water will be:
1. \(\mathrm{74.8~kJ} \mathrm{mol}^{-1}\)
2. \(\mathrm{22.0~kJ} \mathrm{mol}^{-1}\)
3. \(\mathrm{44.1~kJ} \mathrm{mol}^{-1}\)
4. \(\mathrm{52.7kJ} \mathrm{mol}^{-1}\)
| (i) | \(\mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{l})\) \(\Delta \mathrm{H}^{\circ}{ }_{298 \mathrm{~K}}=-285.9 \mathrm{~kJ} \mathrm{~mol}^{-1}\) |
| (ii) | \( \mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{~g}) \) \( \Delta \mathrm{H}^{\circ}{ }_{298 \mathrm{~K}}=-241.8 \mathrm{~kJ} \mathrm{~mol}^{-1}\) |
1. \(\mathrm{74.8~kJ} \mathrm{mol}^{-1}\)
2. \(\mathrm{22.0~kJ} \mathrm{mol}^{-1}\)
3. \(\mathrm{44.1~kJ} \mathrm{mol}^{-1}\)
4. \(\mathrm{52.7kJ} \mathrm{mol}^{-1}\)
Subtopic: Enthalpy & Internal energy |
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What is the boiling point of the liquid at 1 atm if the enthalpy of vaporization of a liquid is 30 \(\mathrm{kJ} \mathrm{mol}^{-1}\) and entropy of vaporization is 75 \( \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\)?
1. 250 \(K\)
2. 400 \(K\)
3. 450 \(K\)
4. 600 \(K\)
1. 250 \(K\)
2. 400 \(K\)
3. 450 \(K\)
4. 600 \(K\)
Subtopic: Spontaneity & Entropy |
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Match the reaction given in column I with appropriate options in column II
1. A-(r, t), B-(p, q, s), C-(p, q, s), D-(p, q, s, t)
2. A-(p, r, s), B-(r, s), C-(t), D-(p, q, t)
3. A-(r, t), B-(p, q,), C-(p, s), D-(p, t)
4. A-(r), B-(s), C-(p), D-(p, q, s, t)
| Column-I (Reaction) |
Column-II (Characteristics/ Property) |
||
| (A) | \( \mathrm{CO}_2(\mathrm{~s}) \rightarrow \mathrm{CO}_2(\mathrm{~g}) \) | (p) | Phase transition |
| (B) | \(\small\mathrm{CaCO}_3(\mathrm{~s}) \rightarrow \mathrm{CaO}(\mathrm{s})+\mathrm{CO}_2(\mathrm{~g})\) | (q) | Allotropic change |
| (C) | \( 2 \mathrm{H}^* \rightarrow \mathrm{H}_2(\mathrm{~g}) \) | (r) | \(\Delta H\) is positive |
| (D) | \( \mathrm{P}_{\text {(white, solid) }} \rightarrow \mathrm{P}_{\text {(red, solid) }} \) | (s) | \(\Delta S\) is positive |
| (t) | \(\Delta S\) is negative |
1. A-(r, t), B-(p, q, s), C-(p, q, s), D-(p, q, s, t)
2. A-(p, r, s), B-(r, s), C-(t), D-(p, q, t)
3. A-(r, t), B-(p, q,), C-(p, s), D-(p, t)
4. A-(r), B-(s), C-(p), D-(p, q, s, t)
Subtopic: Enthalpy & Internal energy | Spontaneity & Entropy |
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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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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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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 (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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