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Q. No.Given below are two statements:
Assertion (A):
Decrease in free energy causes a spontaneous reaction.
Reason (R):
Spontaneous reactions are invariably exothermic reactions.
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.
(A) is False but (R) is True.
Subtopic: Spontaneity & Entropy |
Level 3: 35%-60%
Hints
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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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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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 |
Level 3: 35%-60%
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| Assertion (A): | Enthalpy and entropy of any elementary substance in the standard states are taken as zero. |
| Reason (R): | At absolute zero, particles of the perfectly crystalline substance become completely motionless. |
| 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. | (A) is False but (R) is True. |
Subtopic: 2nd & 3rd Law of Thermodynamics |
Level 4: Below 35%
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Consider the two given statements:
| Assertion (A): | Heat and work are "definite quantities". |
| Reason (R): | Heat and work are not properties of a system their values depend on the path of the process and vary accordingly. |
| 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. | (A) is False but (R) is True. |
Subtopic: Thermodynamics' Properties and process |
Level 3: 35%-60%
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| Assertion (A): | The heat absorbed during the isothermal expansion of an ideal gas against a vacuum is zero. |
| Reason (R): | The volume occupied by the molecules of an ideal gas is zero. |
| 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. | (A) is False but (R) is True. |
Subtopic: Enthalpy & Internal energy |
Level 3: 35%-60%
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At equilibrium, which of the following is always zero?
| 1. | \(\Delta H\) | 2. | \(\Delta S_{Total}\) |
| 3. | \(\Delta S_{System}\) | 4. | \(\Delta G^o\) |
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 |
51%
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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