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Q. No.Maximum work is obtained by a system in:
1.
Irreversible process
2.
Reversible process
3.
Adiabatic process
4.
Isobaric process
Subtopic: First Law of Thermodynamics |
Level 3: 35%-60%
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For an isolated system, if ΔU=0, then what is the value of ΔS?
| 1. | ΔS=0 | 2. | ΔS > 0 |
| 3. | ΔS < 0 | 4. | ΔS is not defined |
Subtopic: Spontaneity & Entropy |
Level 3: 35%-60%
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An ideal gas in a thermally insulated vessel at internal pressure = \(P_1,\) volume = \(V_1,\) and absolute temperature = \(T_1\) expands irreversibly against zero external pressure, as shown in the diagram. The final internal pressure, volume, and absolute temperature of the gas are \(P_2\), \(V_2\) and \(T_2\), respectively.
(b) \( T_2=T_1 \)
(c) \( P_2 V_2=P_1 V_1\)
(d) \(P_2 V_2^\gamma=P_1 V_1^\gamma \)
1. (a), (b) and (c)
2. (b) and (d)
3. (a) and (d)
4. None of the above
Which of the following relation(s) are correct for this expansion?
(a) \(q=0 \)(b) \( T_2=T_1 \)
(c) \( P_2 V_2=P_1 V_1\)
(d) \(P_2 V_2^\gamma=P_1 V_1^\gamma \)
1. (a), (b) and (c)
2. (b) and (d)
3. (a) and (d)
4. None of the above
Subtopic: Thermodynamics' Properties and process |
Level 3: 35%-60%
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For the process
\(\mathrm{H}_2 \mathrm{O}(\mathrm{l})(1 \mathrm{bar}, 373 \mathrm{~K}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g}) (1 \mathrm{bar}, 373 \mathrm{~K})\) , the correct set of thermodynamic parameters is:
1. \( \Delta G=+\mathrm{ve}, \Delta S=0\)
2. \(\Delta G=0, \Delta S=-\mathrm{ve}\)
3. \( \Delta G=0, \Delta S=+\mathrm{ve} \)
4. \( \Delta G=-\mathrm{ve}, \Delta S=+\mathrm{ve} \)
\(\mathrm{H}_2 \mathrm{O}(\mathrm{l})(1 \mathrm{bar}, 373 \mathrm{~K}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g}) (1 \mathrm{bar}, 373 \mathrm{~K})\) , the correct set of thermodynamic parameters is:
1. \( \Delta G=+\mathrm{ve}, \Delta S=0\)
2. \(\Delta G=0, \Delta S=-\mathrm{ve}\)
3. \( \Delta G=0, \Delta S=+\mathrm{ve} \)
4. \( \Delta G=-\mathrm{ve}, \Delta S=+\mathrm{ve} \)
Subtopic: Gibbs Energy Change |
Level 3: 35%-60%
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What is the entropy change (\(\Delta S\)) for water at its boiling point of 100°C, expressed in cal K⁻¹ mol⁻¹?
[For water \(\Delta H_{vap} = 540 ~cal~ g^{-1} \) ]
1. 540
2. 1.45
3. 26.06
4. 35.60
[For water \(\Delta H_{vap} = 540 ~cal~ g^{-1} \) ]
1. 540
2. 1.45
3. 26.06
4. 35.60
Subtopic: Spontaneity & Entropy |
Level 3: 35%-60%
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C2H6(g) + \(\frac{7}{2}\)O2(g) → 2CO2(g) + 3H2O(g) ∆H˚ = –1427.7 kJ
If the enthalpy of vaporization for H2O(l) is 44.0 kJ/mol, Calculate ∆H˚ for this reaction if H2O(l) is formed instead of H2O(g).
1. –1295.7 kJ
2. –1383.7 kJ
3. –1471.7 kJ
4. –1559.7 kJ
If the enthalpy of vaporization for H2O(l) is 44.0 kJ/mol, Calculate ∆H˚ for this reaction if H2O(l) is formed instead of H2O(g).
1. –1295.7 kJ
2. –1383.7 kJ
3. –1471.7 kJ
4. –1559.7 kJ
Subtopic: Hess's Law |
Level 3: 35%-60%
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The enthalpy of combustion of four allotropic forms of element 'X' are given as:
The most stable allotropic form of element 'X' is:
1. A
2. B
3. C
4. D
| Allotropic forms | \(\Delta_\text{comb}H^\circ\)(kJ/mol) |
| A. | -270.3 |
| B. | -189.1 |
| C. | -390.5 |
| D. | -465.0 |
1. A
2. B
3. C
4. D
Subtopic: Thermochemistry |
51%
Level 3: 35%-60%
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At 300K, \(\Delta rG \) and \(\Delta rG^\circ \) are - 12.8 KJ mol-1 and -11.5 KJ mol-1 respectively for the following reaction:
\(A(g) + B(g) \rightleftharpoons C(l) + D(aq)\)
If the reaction is at equilibrium, then the equilibrium constant K will be:
1. \(-2.0 \times 10^0\)
2. \(1.0 \times 10^2\)
3. \(1.0 \times 10^{-2}\)
4. \(1.69 \times 10^0\)
\(A(g) + B(g) \rightleftharpoons C(l) + D(aq)\)
If the reaction is at equilibrium, then the equilibrium constant K will be:
1. \(-2.0 \times 10^0\)
2. \(1.0 \times 10^2\)
3. \(1.0 \times 10^{-2}\)
4. \(1.69 \times 10^0\)
Subtopic: Gibbs Energy Change |
Level 3: 35%-60%
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Consider the given two statements:
Choose the correct answer among the given options:
| Statement I: | A molar property \(\left(X_{\mathrm{m}}\right) \) is the value of an extensive property \(\left(X_{\mathrm{}}\right)\) of the system for 0.1 mol of the substance. |
| Statement II: | If n is the amount of matter, \(X_{\mathrm{m}}=\chi / \mathrm{n}\) is independent of the amount of matter. |
Choose the correct answer among the given options:
| 1. | Statement I is correct; Statement II is correct. |
| 2. | Statement I is incorrect; Statement II is incorrect. |
| 3. | Statement I is correct; Statement II is incorrect. |
| 4. | Statement I is incorrect; Statement II is correct. |
Subtopic: Classification of System, Extensive & Intensive Properties |
Level 3: 35%-60%
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Calculate the standard enthalpy of formation (\(\Delta_fH^\circ\)) for 2 moles of liquid benzene (\(\mathrm{{C_6H_6}_{(l)}}\)) at 25°C, based on the given thermodynamic data.
Given Data:
\(\Delta _c\mathrm H\mathrm{(C_6H_6}_\mathrm{(l)})~= -3264.6~ \mathrm{~kJ} / \mathrm{mol}\)
\(\Delta _c\mathrm H\mathrm{(C}_\mathrm{(s)})~= -393.5~ \mathrm{~kJ} / \mathrm{mol}\)
\(\Delta _f\mathrm H\mathrm{(H_2O}_\mathrm{(l)})~= -285.83~ \mathrm{~kJ} / \mathrm{mol}\)
1. \(-~92.22 \mathrm{~kJ} / \mathrm{mol}\)
2. \(-46.11 \mathrm{~kJ} / \mathrm{mol}\)
3. \(+~92.22 \mathrm{~kJ} / \mathrm{mol}\)
4. \(+46.11 \mathrm{~kJ} / \mathrm{mol}\)
Given Data:
\(\Delta _c\mathrm H\mathrm{(C_6H_6}_\mathrm{(l)})~= -3264.6~ \mathrm{~kJ} / \mathrm{mol}\)
\(\Delta _c\mathrm H\mathrm{(C}_\mathrm{(s)})~= -393.5~ \mathrm{~kJ} / \mathrm{mol}\)
\(\Delta _f\mathrm H\mathrm{(H_2O}_\mathrm{(l)})~= -285.83~ \mathrm{~kJ} / \mathrm{mol}\)
1. \(-~92.22 \mathrm{~kJ} / \mathrm{mol}\)
2. \(-46.11 \mathrm{~kJ} / \mathrm{mol}\)
3. \(+~92.22 \mathrm{~kJ} / \mathrm{mol}\)
4. \(+46.11 \mathrm{~kJ} / \mathrm{mol}\)
Subtopic: Thermochemistry |
Level 3: 35%-60%
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