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Q. No.From the given data, find the enthalpy of hydrogenation of ethene in kJ/mol.
(a) B.E. of C – C = 350 kJ/mol
(b) B.E. of C = C = 600 kJ/mol
(c) B.E. of H – H = 400 kJ/mol
(d) B.E. of C – H = 410 kJ/mol
1. –170
2. –580
3. +170
4. +580
Subtopic: Thermochemistry |
79%
Level 2: 60%+
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Calculate the magnitude of heat (q) in joules for an isothermal irreversible expansion, where the system expands against an external pressure of 8 bar, and the volume increases by 10 L.
| 1. | 8000 J | 2. | 2000 J |
| 3. | 6000 J | 4. | 7600 J |
Subtopic: First Law of Thermodynamics |
90%
Level 1: 80%+
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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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Find out work done on the gas for following process :
1. \(61.5 \text { Joule }\)
2. \(-61.5 \text { Joule }\)
3. \(\text { +246 Joule }\)
4. \(\text { -246 Joule }\)
1. \(61.5 \text { Joule }\)
2. \(-61.5 \text { Joule }\)
3. \(\text { +246 Joule }\)
4. \(\text { -246 Joule }\)
Subtopic: First Law of Thermodynamics |
61%
Level 2: 60%+
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For a certain reaction, if \(\Delta_{\mathrm{r}} \mathrm{H}\) is \(400 \mathrm{~kJ} / \mathrm{mol}\) and \(\Delta \mathrm{S}=0.2 \mathrm{~kJ} / \mathrm{mol}\), calculate the minimum temperature (in Kelvin) at which the reaction becomes spontaneous.
1. 1000
2. 2000
3. 4000
4. 100
1. 1000
2. 2000
3. 4000
4. 100
Subtopic: Spontaneity & Entropy |
92%
Level 1: 80%+
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A mixture contains one mole of a monoatomic gas and one mole of a diatomic gas. What is the ratio of the heat capacities at constant volume (\(C_V\)) to the heat capacities at constant pressure (\(C_P\)) for the mixture\(\left(\text { i.e. } \frac{C_v}{C_P}\right)\)?
| 1. | \(\dfrac{2}{3}\) | 2. | \(\dfrac{7}{5}\) |
| 3. | \(\dfrac{5}{7}\) | 4. | \(\dfrac{3}{5}\) |
Subtopic: Cp & Cv |
64%
Level 2: 60%+
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Calculate the magnitude of work done on the gas at \(18^{\circ} \mathrm{C}\) ,when 1 mole of an ideal gas undergoes compression from 9 litre to 1 litre through a reversible isothermal process:
(Take log3 = 0.48)
1. 5349 J
2. 1789 J
3. 8902 J
4. 7690 J
(Take log3 = 0.48)
1. 5349 J
2. 1789 J
3. 8902 J
4. 7690 J
Subtopic: First Law of Thermodynamics |
84%
Level 1: 80%+
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A 1 mol ideal gas expands from 10 L to 100 L at 300 K, If the above expansion takes place reversibly and isothermally, then the magnitude of work done is:
1. 6 KJ
2. 9 KJ
3. 4 KJ
4. 5 KJ
1. 6 KJ
2. 9 KJ
3. 4 KJ
4. 5 KJ
Subtopic: First Law of Thermodynamics |
81%
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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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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