Q. No.Match the entries in Column-I with those given in Column-II:
1. A-q, B-p, C-r, D-s
2. A-p, B-q, C-r, D-s
3. A-s, B-q, C-r, D-p
4. A-q, B-s, C-r, D-q
| Column-I | Column-II | ||
| (A) | Reversible process | (p) | \(\Delta G = -nFE\) |
| (B) | Gibbs free energy | (q) | Infinite steps |
| (C) | Standard enthalpy of reaction, \(\Delta_r H^{\ominus}\) | (r) | \(\sum\)bond enthalpies (reactants) – \(\sum\)bond enthalpies (products) |
| (D) | Enthalpy of bond formation, \(\Delta_f H_{\text {bond }}^{\ominus}\) | (s) | \(\sum \Delta_f H^{\ominus}\)(bonds of products) – \(\sum \Delta_f H^{\ominus}\)(bonds of reactants) |
2. A-p, B-q, C-r, D-s
3. A-s, B-q, C-r, D-p
4. A-q, B-s, C-r, D-q
Subtopic: Gibbs Energy Change | Thermochemistry |
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Level 1: 80%+
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Identify correct match using Column I & Column II
| Column I | Column II | ||
| (i) | Spontaneous process | (a) | Isothermal and isobaric process |
| (ii) | \(\Delta H^\circ\) | (b) | \(\Delta H<0 \) |
| (iii) | \(\Delta T=0, \Delta P=0 \) | (c) | \(\Delta G<0 \) |
| (iv) | Exothermic process | (d) | (Bond energy of reactant) - (Bond energy of product) |
| I | II | III | IV | |
| 1. | c | d | a | b |
| 2. | b | a | c | d |
| 3. | d | b | c | d |
| 4. | a | d | b | c |
Subtopic: First Law of Thermodynamics | Spontaneity & Entropy | Gibbs Energy Change |
94%
Level 1: 80%+
JEE
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Tin is obtained from cassiterite by reduction with coke. What is the minimum temperature (in K) at which the reduction of cassiterite by coke would take place?
[Note: Assume that the enthalpies and the entropies are temperature-independent]
\(\text{Given:}~\text{At } 298 \mathrm{~K} ;\)
\(\Delta H^0\left(\mathrm{SnO}_2(s)\right)=-581.0 \mathrm{~kJ} \mathrm{~mol}^{-1}, \\\Delta_f H^0\left(\mathrm{CO}_2(g)\right)=-394.0 \mathrm{~kJ} \mathrm{~mol}^{-1}, \)
\(S^0\left(\mathrm{SnO}_2(s)\right)=56.0 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}, \\S^0(\mathrm{Sn}(s))=52.0 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\)
\( S^0(\mathrm{C}(s))=6.0 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}, \\S^0\left(\mathrm{CO}_2(g)\right)=210.0 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\)
Choose the correct option:
1. 735 K
2. 303 K
3. 935 K
4. 456 K
[Note: Assume that the enthalpies and the entropies are temperature-independent]
\(\text{Given:}~\text{At } 298 \mathrm{~K} ;\)
\(\Delta H^0\left(\mathrm{SnO}_2(s)\right)=-581.0 \mathrm{~kJ} \mathrm{~mol}^{-1}, \\\Delta_f H^0\left(\mathrm{CO}_2(g)\right)=-394.0 \mathrm{~kJ} \mathrm{~mol}^{-1}, \)
\(S^0\left(\mathrm{SnO}_2(s)\right)=56.0 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}, \\S^0(\mathrm{Sn}(s))=52.0 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\)
\( S^0(\mathrm{C}(s))=6.0 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}, \\S^0\left(\mathrm{CO}_2(g)\right)=210.0 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\)
Choose the correct option:
1. 735 K
2. 303 K
3. 935 K
4. 456 K
Subtopic: Spontaneity & Entropy | Gibbs Energy Change |
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Hydrolysis of sucrose is given by the following reaction
Sucrose + H2O Glucose + Fructose
If the equilibrium constant (Kc) is 21013 at 300 K, the value of at the same temperature will be:
1. 8.314 J mol-1 K-1300 Kln (21013)
2. 8.314 J mol-1 K-1300 Kln (31013)
3. -8.314 J mol-1 K-1300 Kln (41013)
4. -8.314 J mol-1 K-1300 Kln (21013)
Subtopic: Gibbs Energy Change |
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Level 1: 80%+
NEET - 2020
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The free energy change due to a reaction is zero when :
| 1. | The reactants are initially mixed |
| 2. | A catalyst is added |
| 3. | The system is at an equilibrium |
| 4. | The reactants are completely consumed |
Subtopic: Gibbs Energy Change |
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Which of the following is the maximum energy available for useful work from a spontaneous reaction?
| 1. | Gibbs free energy | 2. | Lattice energy |
| 3. | Kinetic energy | 4. | Ionization energy |
Subtopic: Gibbs Energy Change |
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The standard enthalpy and entropy changes of decomposition of N2O4 to NO2 are 55.0 kJmol–1 and 175.0 JK–1 mol–1 respectively. The standard free energy change for this reaction at 25°C in J mol–1 is:
| 1. | 2750 | 2. | 2850 |
| 3. | 2875 | 4. | 2900 |
Subtopic: Spontaneity & Entropy | Gibbs Energy Change |
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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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Level 1: 80%+
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The correct thermodynamic conditions for a spontaneous reaction at all temperatures is:
1. H > 0 and S< 0
2. H < 0 and S> 0
3. H < 0 and S< 0
4. H > 0 and S = 0
1. H > 0 and S< 0
2. H < 0 and S> 0
3. H < 0 and S< 0
4. H > 0 and S = 0
Subtopic: Gibbs Energy Change |
85%
Level 1: 80%+
NEET - 2016
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The enthalpy and entropy change for a chemical reaction are
–2.5 × 103 cal and 7.4 cal deg–1 respectively. Predict the reaction at 298 K is
1. Spontaneous
2. Reversible
3. Irreversible
4. Non-spontaneous
Subtopic: Gibbs Energy Change |
84%
Level 1: 80%+
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