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Q. No.What is the value of enthalpy change \( (\Delta\text{H})\) (in kJ/mole) for the given reaction?
\(3 \mathrm{C}(\mathrm{s})+\mathrm{Fe}_2 \mathrm{O}_3(\mathrm{~s}) \rightarrow 2 \mathrm{Fe}(\mathrm{s})+3 \mathrm{CO}(\mathrm{g})\)
Given :
\(\begin{aligned} & 2 \mathrm{Fe}(\mathrm{s})+\frac{3}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{Fe}_2 \mathrm{O}_3(\mathrm{~s}) \Delta \mathrm{H}^{\circ}=-824 \mathrm{~kJ} / \mathrm{mol} \\ & \mathrm{C}(\mathrm{s})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{CO}(\mathrm{g}) \Delta \mathrm{H}^{\circ}=-110 \mathrm{~kJ} / \mathrm{mol} \end{aligned}\)
1. 494
2. 984
3. 700
4. 560
Subtopic: Thermochemistry |
95%
Level 1: 80%+
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Calculate the relationship between the heat released when dilute NaOH completely neutralises equal volumes of 1 M HCl and 1 M H₂SO₄. If the heat released is x and y kcal mol⁻¹ respectively, find the correct interpretation.
1. x = y
2. x = 0.5y
3. x = 0.4y
4. x = 2y
Subtopic: Thermochemistry |
68%
Level 2: 60%+
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Find the value of x for the hydration reaction:
CuSO₄(s) + 5H₂O(l) → CuSO₄·5H₂O(s)
Given:
Heat of solution of CuSO₄ = –70 kJ mol⁻¹
Heat of solution of CuSO₄·5H₂O = +12 kJ mol⁻¹
ΔH(hydration) = –x kJ mol⁻¹
1. 82
2. 98
2. 67
4. 90
Subtopic: Thermochemistry |
90%
Level 1: 80%+
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Subtopic: Thermodynamics' Properties and process |
77%
Level 2: 60%+
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What is the work done on the gas in cyclic process ABCA ?
1. \( +773.7 \mathrm{~J}\)
2. \(-773.7 \mathrm{~J}\)
3. \(+4762.3 \mathrm{~J} \)
4. \(-4762.3 \mathrm{~J}\)
Subtopic: First Law of Thermodynamics |
56%
Level 3: 35%-60%
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Hints
Which of the following statement is incorrect?
1. \(\triangle\text{G}=0\) for reversible process
2. \(\triangle\text{G}<0\) for spontaneous process
3. \(\triangle\text{G}>0\) for spontaneous process
4. \(\triangle\text{G}>0\) for non-spontaneous process
1. \(\triangle\text{G}=0\) for reversible process
2. \(\triangle\text{G}<0\) for spontaneous process
3. \(\triangle\text{G}>0\) for spontaneous process
4. \(\triangle\text{G}>0\) for non-spontaneous process
Subtopic: Gibbs Energy Change |
92%
Level 1: 80%+
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If the standard enthalpy of vaporization of \( \text{CCl}_4\) is 30.5 kJ/mol, find heat absorbed for vaporization of 294 gm of \( \text{CCl}_4.\)
1. 78 KJ
2. 58 KJ
3. 100 KJ
4. 80 KJ
1. 78 KJ
2. 58 KJ
3. 100 KJ
4. 80 KJ
Subtopic: Thermochemistry |
94%
Level 1: 80%+
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Given that the values of ΔH° and ΔS° for a process/reaction are 77.2 kJ and 48 J/K, respectively, calculate the value of log 1/k when the temperature is 300 K.
1. 11
2. 5
3. 15
4. 100
1. 11
2. 5
3. 15
4. 100
Subtopic: Enthalpy & Internal energy |
63%
Level 2: 60%+
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Calculate the molar heat capacity at constant volume, Cᵥ,ₘ, of a gaseous mixture containing 2 moles of a monoatomic gas and 6 moles of a diatomic gas.
Given:
For monoatomic gas, Cᵥ,ₘ = 3R/2
For diatomic gas, Cᵥ,ₘ = 5R/2
1. 9R/42. 9R/2
3. 3R
4. 4R
Subtopic: Cp & Cv |
87%
Level 1: 80%+
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Hints
Which of the following is correct for adiabatic free expansion against vacuum?
1. \(\mathrm{q}=0, \Delta \mathrm{U}=0, \mathrm{~W}=0\)
2. \(\mathrm{q} \neq 0, \mathrm{~W}=0, \Delta \mathrm{U}=0\)
3. \(\mathrm{q}=0, \Delta \mathrm{U} \neq 0, \mathrm{~W}=0\)
4. \(q=0, \Delta U \neq 0, W \neq 0\)
1. \(\mathrm{q}=0, \Delta \mathrm{U}=0, \mathrm{~W}=0\)
2. \(\mathrm{q} \neq 0, \mathrm{~W}=0, \Delta \mathrm{U}=0\)
3. \(\mathrm{q}=0, \Delta \mathrm{U} \neq 0, \mathrm{~W}=0\)
4. \(q=0, \Delta U \neq 0, W \neq 0\)
Subtopic: First Law of Thermodynamics |
95%
Level 1: 80%+
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