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Q. No.Match List-I with List-II:
List-I
List-II
(A)
Spontaneous process
(I)
\(\mathrm{\Delta H<0}\)
(B)
Process with \(\mathrm{\Delta P=0,} \mathrm{\Delta T=0}\)
(II)
\(\mathrm{\Delta G_{T,P}<0}\)
(C)
\(\mathrm{\Delta H_{reaction}}\)
(III)
Isothermal and Isobaric processes
(D)
Exothermic Process
(IV)
[Bond energies of molecules in reactants] – [Bond energies of molecules in reactants]
Choose the correct answer from the options given below:
1. (A)-(III), (B)-(II), (C)-(IV), (D)-(I)
2. (A)-(II), (B)-(III), (C)-(IV), (D)-(I)
3. (A)-(II), (B)-(III), (C)-(I), (D)-(IV)
4. (A)-(II), (B)-(I), (C)-(III), (D)-(IV)
Subtopic: Thermodynamics' Properties and process |
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Level 1: 80%+
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What is the amount of heat absorbed in the expansion of an ideal gas from \(\mathrm{4.0 ~L}\) to \(\mathrm{20~ L}\) when the gas is allowed to expand isothermally into a vacuum:
1. 20 \(\mathrm{L}\) atm
2. 0 \(\mathrm{L}\) atm
3. 40 \(\mathrm{L}\) atm
4. 24 \(\mathrm{L}\) atm
1. 20 \(\mathrm{L}\) atm
2. 0 \(\mathrm{L}\) atm
3. 40 \(\mathrm{L}\) atm
4. 24 \(\mathrm{L}\) atm
Subtopic: First Law of Thermodynamics |
90%
Level 1: 80%+
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The magnitude of work done by a gas during a reversible expansion along the path ABC, as shown in the figure, is:
| 1. | 44 Nm | 2. | 46 Nm |
| 3. | 48 Nm | 4. | 50 Nm |
Subtopic: Thermodynamics' Properties and process | First Law of Thermodynamics |
82%
Level 1: 80%+
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For a given chemical reaction A ⇌ B at \(\text 300 ~ \text K\), the free energy change is \(– 49.4~\mathrm{kJ ~mol^{–1}}\) and the enthalpy of reaction is \(51.4~\mathrm{kJ~ mol^{–1} }\). The entropy change of the reaction is:
1. \(140 ~\mathrm{JK^{–1} mol^{–1}}\)
2. \(671~\mathrm{JK^{–1} mol^{–1}}\)
3. \(336~\mathrm{JK^{–1} mol^{–1}}\)
4. \(390 ~\mathrm{JK^{–1} mol^{–1}}\)
1. \(140 ~\mathrm{JK^{–1} mol^{–1}}\)
2. \(671~\mathrm{JK^{–1} mol^{–1}}\)
3. \(336~\mathrm{JK^{–1} mol^{–1}}\)
4. \(390 ~\mathrm{JK^{–1} mol^{–1}}\)
Subtopic: Gibbs Energy Change |
83%
Level 1: 80%+
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During which of the following processes, does entropy decrease?
Choose the correct option among the following:
1. (A), (B), (C) and (D) only
2. (B) and (C) only
3. (A), (C) and (E) only
4. (A) and (E) only
| (A) | Freezing of water to ice at \(0^\circ C\) |
| (B) | Freezing of water to ice at \(-10^\circ C\) |
| (C) | \(\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightarrow 2 \mathrm{NH}_3(\mathrm{~g})\) |
| (D) | Adsorption of CO(g) on lead surface |
| (E) | Dissolution of NaCl in water |
Choose the correct option among the following:
1. (A), (B), (C) and (D) only
2. (B) and (C) only
3. (A), (C) and (E) only
4. (A) and (E) only
Subtopic: Spontaneity & Entropy |
82%
Level 1: 80%+
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Consider the given reaction:
\(3{CaO}+2{Al} \longrightarrow 3{Ca}+{Al}_2 \mathrm{O}_3\)
The standard enthalpies of formation of \(Al_2O_3~ \text{and}~ CaO~ \text{are}~ –1675 ~kJ~ mol^{–1}\) and \(–635~ kJ ~mol^{–1}\) respectively.
Calculate the standard reaction enthalpy (\(\Delta_ rH^0\)) for this reaction:
1. \(1230 ~\mathrm{kJ} \)
2. \(43 ~ \mathrm{kJ} \)
3. \(230~ \mathrm{kJ} \)
4. \(312~ \mathrm{kJ} \)
\(3{CaO}+2{Al} \longrightarrow 3{Ca}+{Al}_2 \mathrm{O}_3\)
The standard enthalpies of formation of \(Al_2O_3~ \text{and}~ CaO~ \text{are}~ –1675 ~kJ~ mol^{–1}\) and \(–635~ kJ ~mol^{–1}\) respectively.
Calculate the standard reaction enthalpy (\(\Delta_ rH^0\)) for this reaction:
1. \(1230 ~\mathrm{kJ} \)
2. \(43 ~ \mathrm{kJ} \)
3. \(230~ \mathrm{kJ} \)
4. \(312~ \mathrm{kJ} \)
Subtopic: Enthalpy & Internal energy |
83%
Level 1: 80%+
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The following reactions were carried out in an open vessel. The reaction for which \(\mathrm{\Delta H= \Delta U}\) will be:
1. \(\mathrm{PCl}_5(\mathrm{~g}) \rightarrow \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})\)
2. \(2 \mathrm{CO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{CO}_2(\mathrm{~g})\)
3. \(\text 3\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightarrow 2 \mathrm{NH}_3(\mathrm{~g})\)
4. \(\mathrm{H}_2(\mathrm{~g})+\mathrm{I}_2(\mathrm{~g}) \rightarrow 2 \mathrm{HI}(\mathrm{g})\)
1. \(\mathrm{PCl}_5(\mathrm{~g}) \rightarrow \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})\)
2. \(2 \mathrm{CO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{CO}_2(\mathrm{~g})\)
3. \(\text 3\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightarrow 2 \mathrm{NH}_3(\mathrm{~g})\)
4. \(\mathrm{H}_2(\mathrm{~g})+\mathrm{I}_2(\mathrm{~g}) \rightarrow 2 \mathrm{HI}(\mathrm{g})\)
Subtopic: Enthalpy & Internal energy |
90%
Level 1: 80%+
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What is the enthalpy change (ΔH) for the following reaction?
\(\mathrm {H}_2 \mathrm{C} = \mathrm {CH}_2 \text {(g)}+\mathrm{H}_2 \text {(g)} \rightarrow\mathrm {H}_3 \mathrm {C} - \mathrm {CH}_3 \text {(g)}\)
(Use the following bond energy data:
H-C: 413 kJ/mole
H-H: 436 kJ/mole
C=C: 614 kJ/mole
C-C: 348 kJ/ mole )
1. -656 kJ/mole
2. -343 kJ/mole
3. -289 kJ/mole
4. -124 kJ/mole
\(\mathrm {H}_2 \mathrm{C} = \mathrm {CH}_2 \text {(g)}+\mathrm{H}_2 \text {(g)} \rightarrow\mathrm {H}_3 \mathrm {C} - \mathrm {CH}_3 \text {(g)}\)
(Use the following bond energy data:
H-C: 413 kJ/mole
H-H: 436 kJ/mole
C=C: 614 kJ/mole
C-C: 348 kJ/ mole )
1. -656 kJ/mole
2. -343 kJ/mole
3. -289 kJ/mole
4. -124 kJ/mole
Subtopic: Thermochemistry |
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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 |
88%
Level 1: 80%+
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Given the following reaction:
\(\mathrm{C}_2 \mathrm{H}_4(g)+6 \mathrm{~F}_2(g) \rightarrow 2 \mathrm{CF}_4(g)+4 \mathrm{HF}(g)\)
Which species has a standard enthalpy of formation \((\Delta H^{\circ})\) equal to 0?
1. \(\mathrm{C}_2 \mathrm{H}_4\)
2. \(\mathrm{F}_2\)
3. \(\mathrm{CF}_4\)
4. \(\mathrm{HF}\)
\(\mathrm{C}_2 \mathrm{H}_4(g)+6 \mathrm{~F}_2(g) \rightarrow 2 \mathrm{CF}_4(g)+4 \mathrm{HF}(g)\)
Which species has a standard enthalpy of formation \((\Delta H^{\circ})\) equal to 0?
1. \(\mathrm{C}_2 \mathrm{H}_4\)
2. \(\mathrm{F}_2\)
3. \(\mathrm{CF}_4\)
4. \(\mathrm{HF}\)
Subtopic: Thermochemistry |
84%
Level 1: 80%+
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