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Q. No.One mole of a gas is undergoing following process, in which of the following work done by the gas is maximum?
| 1. |  |
| 2. |  |
| 3. |  |
| 4. |  |
Subtopic: First Law of Thermodynamics |
Level 4: Below 35%
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Hints
For the reaction : \(A_2 + B_2 \xrightarrow {500~K} 2 AB\) : where, Log K = 2.2
Calculate the value of x:
1. 70
2. 60
3. 50
4. 80
| \(\mathrm{H}_{\mathrm{f}}{ }^0 \text { (KJ/mole) }\) | \(\mathrm{S}_{\mathrm{f}}^0(\mathrm{~J} / \mathrm{K} \text {-mole })\) | |
| AB | 32 | 240 |
| \(A_2\) | 6 | 224 |
| \(B_2\) | x | 238 |
Calculate the value of x:
1. 70
2. 60
3. 50
4. 80
Subtopic: Enthalpy & Internal energy | Spontaneity & Entropy |
Level 4: Below 35%
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Hints
Ten moles of oxygen gas (O₂) are heated at constant volume, causing the temperature to increase from 30°C to 40°C. Calculate the change in internal energy of the gas (in calories):
[Given: \(\mathrm{C}_p=7 \frac{\mathrm{Cal}}{\mathrm{~mol}-\mathrm{K}};~ \mathrm{R}=2 \frac{\mathrm{Cal}}{\mathrm{~mol}-\mathrm{K}}\)]
1. 400
2. 500
3. 600
4. 700
[Given: \(\mathrm{C}_p=7 \frac{\mathrm{Cal}}{\mathrm{~mol}-\mathrm{K}};~ \mathrm{R}=2 \frac{\mathrm{Cal}}{\mathrm{~mol}-\mathrm{K}}\)]
1. 400
2. 500
3. 600
4. 700
Subtopic: Cp & Cv |
Level 4: Below 35%
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Hints
Calculate Bond Energy of C-H bond in \(CH_4\):
Given: \(\Delta H_r\) of \(CH_4(g) = -\text {x kJ/mol}\)
\(\Delta H_{sub}\) of carbon = y kJ/mol
B.E. of H-H=z kJ/mol
1. \(\frac{x-y+z}{4} \)
2. \(\frac{y+2 z+x}{4} \)
3. \(\frac{y-2 z-x}{4} \)
4. \(\frac{2 y-z+x}{4}\)
Given: \(\Delta H_r\) of \(CH_4(g) = -\text {x kJ/mol}\)
\(\Delta H_{sub}\) of carbon = y kJ/mol
B.E. of H-H=z kJ/mol
1. \(\frac{x-y+z}{4} \)
2. \(\frac{y+2 z+x}{4} \)
3. \(\frac{y-2 z-x}{4} \)
4. \(\frac{2 y-z+x}{4}\)
Subtopic: Hess's Law |
Level 4: Below 35%
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Hints
4 kg of water is heated from \(4^\circ C\) to \(20^\circ C\) at constant pressure \(10^5\) Pa, so that density changes from \(1000~kg/m^3\) to \(998 ~kg/m^3.\) Then find \(\Delta U\) (in Joules ):
[Given: \(C_s\) of \(H_2O=4.2 \) Joule /gm.K]
1. 268799.2 Joule
2. 368900 Joule
3. 168400 Joule
4. 578876.8 Joule
[Given: \(C_s\) of \(H_2O=4.2 \) Joule /gm.K]
1. 268799.2 Joule
2. 368900 Joule
3. 168400 Joule
4. 578876.8 Joule
Subtopic: Enthalpy & Internal energy |
Level 4: Below 35%
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Hints
| List -I (Isothermal Process) |
List-II (work done) \((V_f>V_i)\) |
||
| P | Reversible expansion | 1. | \(w=0\) |
| Q | Free expansion | 2. | \(w=-n R T \ln \frac{V_f}{V_i}\) |
| R | Irreversible expansion | 3. | \(w=-\mathrm{P}_{\mathrm{ext}}\left(\mathrm{~V}_{\mathrm{f}}-\mathrm{V}_{\mathrm{i}}\right)\) |
| S | Irreversible Compression |
4. | \(\mathrm{w}=-\mathrm{P}_{\mathrm{ext}}\left(\mathrm{~V}_{\mathrm{i}}-\mathrm{V}_{\mathrm{f}}\right)\) |
Select the correct match:
| P | Q | R | S | |
| 1. | 4 | 3 | 2 | 1 |
| 2. | 2 | 1 | 3 | 4 |
| 3. | 1 | 2 | 3 | 4 |
| 4. | 3 | 4 | 1 | 2 |
Subtopic: Thermodynamics' Properties and process |
Level 4: Below 35%
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Hints
Find the magnitude of lattice energy of LiF (in kJ/mol):
Given :
Enthalpy of sublimation of Li(s) = 161 kJ/mol
Ionisation enthalpy of Li(g) = 520 kJ/mol
Bond Enthalpy of \(F_2\) (g) = 154 kJ/mol
Electron gain enthalpy of F(g) = –328 kJ/mol
Enthalpy of formation of LiF(s) = – 617 kJ/mol
1. -947
2. -1047
3. +956
4. +1097
Given :
Enthalpy of sublimation of Li(s) = 161 kJ/mol
Ionisation enthalpy of Li(g) = 520 kJ/mol
Bond Enthalpy of \(F_2\) (g) = 154 kJ/mol
Electron gain enthalpy of F(g) = –328 kJ/mol
Enthalpy of formation of LiF(s) = – 617 kJ/mol
1. -947
2. -1047
3. +956
4. +1097
Subtopic: Hess's Law | Thermochemistry |
68%
Level 2: 60%+
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Hints
For an ideal gas volume is made 8 times and temperature is decreased 4 times, and heat exchanged during process is zero (q=0), select the correct gas:
1. \(CH_4\)
2. \(He\)
3. \(CO_2\)
4. \(NH_3\)
1. \(CH_4\)
2. \(He\)
3. \(CO_2\)
4. \(NH_3\)
Subtopic: Thermodynamics' Properties and process |
77%
Level 2: 60%+
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Hints
| List-I | List-II (KJ) |
||
| (I) | Isothermal reversible (1mole ideal gas, T = 300K, \(2dm^3\) to \(20dm^3 ) \)calculate |w| | (A) | 8.32 |
| (II) | Isothermal irreversible \([3KPa, 1m^3 ~\text{to} ~3m^3 ]\) calculate |w| | (B) | 6 |
| (III) | 1 mole gas undergoes constant pressure process in which change in temperature is 400K, Cp = 5R/2, calculate \(\Delta H\) | (C) | 4 |
| (IV) | 1 mole ideal gas having Cv=3R/2 and \(\Delta T\) = 320K, calculate \(\Delta U\) | (D) | 5.74 |
Select the correct match
1. I-A: II-B: III-D: IV-C
2. I-D: II-B: III-A: IV-C
3. I-B: II-A: III-C: IV-D
4. I-A: II-B: III-C: IV-D
Subtopic: Thermodynamics' Properties and process | Enthalpy & Internal energy |
90%
Level 1: 80%+
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Hints
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For the following change:
\(\begin{aligned} & \mathrm{H}_2 \mathrm{O}(\ell) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{~g}) \\ & 5^{\circ} \mathrm{C} \quad 100^{\circ} \mathrm{C} \end{aligned}\)
Choose the correct answer:
1. \( \mathrm{q}=+\mathrm{ve}, \mathrm{w}=+\mathrm{ve}, \Delta \mathrm{U}=+\mathrm{ve} \)
2. \( \mathrm{q}=-\mathrm{ve}, \mathrm{w}=-\mathrm{ve}, \Delta \mathrm{U}=+\mathrm{ve} \)
3. \(\mathrm{q}=+\mathrm{ve}, \mathrm{w}=-\mathrm{ve}, \Delta \mathrm{U}=+\mathrm{ve} \)
4. \( \mathrm{q}=-\mathrm{ve}, \mathrm{w}=-\mathrm{ve}, \Delta \mathrm{U}=-\mathrm{ve}\)
\(\begin{aligned} & \mathrm{H}_2 \mathrm{O}(\ell) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{~g}) \\ & 5^{\circ} \mathrm{C} \quad 100^{\circ} \mathrm{C} \end{aligned}\)
Choose the correct answer:
1. \( \mathrm{q}=+\mathrm{ve}, \mathrm{w}=+\mathrm{ve}, \Delta \mathrm{U}=+\mathrm{ve} \)
2. \( \mathrm{q}=-\mathrm{ve}, \mathrm{w}=-\mathrm{ve}, \Delta \mathrm{U}=+\mathrm{ve} \)
3. \(\mathrm{q}=+\mathrm{ve}, \mathrm{w}=-\mathrm{ve}, \Delta \mathrm{U}=+\mathrm{ve} \)
4. \( \mathrm{q}=-\mathrm{ve}, \mathrm{w}=-\mathrm{ve}, \Delta \mathrm{U}=-\mathrm{ve}\)
Subtopic: Thermodynamics' Properties and process | First Law of Thermodynamics |
56%
Level 3: 35%-60%
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Hints
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