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Q. No.An athlete is given 100 g of glucose energy equivalent to 1560 kJ to utilize 50 % of this gained energy in an event. Enthalpy of evaporation of H2O is 44 kJ/mol. In order to avoid storage of energy in the body the mass of water (in g) he would perspire is:
(Round off the nearest Integer)
1. 325 g
2. 319 g
3. 298 g
4. 345 g
Subtopic: Thermochemistry |
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Level 2: 60%+
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For independent processes at 300 K.
\(\begin{array}{|c|c|c|} \hline \text { Process } & \Delta \mathbf{H} / \mathbf{k J} \mathrm{mol}^{-1} & \Delta \mathbf{S} / \mathrm{J} \mathrm{K}^{-1} \\ \hline \text { A } & -25 & -80 \\ \hline \text { B } & -22 & 40 \\ \hline \mathrm{C} & 25 & -50 \\ \hline \text { D } & 22 & 20 \\ \hline \end{array} \)
How many of the above process(es) are non-spontaneous?
1. 2 processes
2. 3 processes
3. 1 process
4. 4 process
\(\begin{array}{|c|c|c|} \hline \text { Process } & \Delta \mathbf{H} / \mathbf{k J} \mathrm{mol}^{-1} & \Delta \mathbf{S} / \mathrm{J} \mathrm{K}^{-1} \\ \hline \text { A } & -25 & -80 \\ \hline \text { B } & -22 & 40 \\ \hline \mathrm{C} & 25 & -50 \\ \hline \text { D } & 22 & 20 \\ \hline \end{array} \)
How many of the above process(es) are non-spontaneous?
1. 2 processes
2. 3 processes
3. 1 process
4. 4 process
Subtopic: Gibbs Energy Change |
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Level 2: 60%+
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If the volume of an ideal gas is increased isothermally then its internal energy will be:
1. Increases
2. Remains constant
3. Decreases
4. Can be increased or decreased
1. Increases
2. Remains constant
3. Decreases
4. Can be increased or decreased
Subtopic: First Law of Thermodynamics |
85%
Level 1: 80%+
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The correct match for the following options is:
1. A → Q, B → P, C → S, D → R
2. A → P, B → Q, C → R, D → S
3. A → S, B → R, C → Q, D → P
4. A → P, B → R, C → S, D → Q
| List-I | List-II | ||
| (A) | Adiabatic | (P) | ∆T = 0 |
| (B) | Isothermal | (Q) | Heat exchange is zero |
| (C) | Isochoric | (R) | ∆P = 0 |
| (D) | Isobaric | (S) | Work done is zero |
1. A → Q, B → P, C → S, D → R
2. A → P, B → Q, C → R, D → S
3. A → S, B → R, C → Q, D → P
4. A → P, B → R, C → S, D → Q
Subtopic: First Law of Thermodynamics |
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Level 1: 80%+
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| Assertion (A): | The first law of thermodynamics has the equation: ∆U = q + W |
| Reason (R): | The first law of thermodynamics is based on the law of conservation of energy. |
| 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. | Both (A) and (R) are False. |
Subtopic: First Law of Thermodynamics |
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Level 1: 80%+
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Calculate the value of x if the heat of reaction measured in a bomb calorimeter for the reaction:
CH₃OH(l) + 3/2 O₂(g) → CO₂(g) + 2H₂O(l)
is −786 kJ at 27°C.
1. 787
2. 797
3. 778
4. 810
Subtopic: Enthalpy & Internal energy |
81%
Level 1: 80%+
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A container of fixed volume filled with an ideal gas which have \(\frac{C_P}{C_V}=1.4,\) is moving with velocity 'v' and then suddenly stopped. If no heat loss is observed, then the final increase in temperature is: (M=Molar mass of gas).
1. \(\frac{Mv^2}{7R}\)
2. \(\frac{2Mv^2}{7R}\)
3. \(\frac{2Mv^2}{5R}\)
4. \(\frac{Mv^2}{5R}\)
1. \(\frac{Mv^2}{7R}\)
2. \(\frac{2Mv^2}{7R}\)
3. \(\frac{2Mv^2}{5R}\)
4. \(\frac{Mv^2}{5R}\)
Subtopic: Cp & Cv |
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Level 3: 35%-60%
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A fish swimming in a water body when taken out from the water body is covered with a film of water of weight 36 g. When it is subjected to cooking at 100°C, then the internal energy for vaporization is:
[Assume steam to be an ideal gas. Given \(\Delta_\text{vap}H^{\ominus} \) for water at 373 K and 1 bar is 41.1 kJ mol-1; R=8.31 JK-1 mol-1 ]
1. 38 kJ/mol
2. 42 kJ/mol
3. 35 kJ/mol
4. 33 kJ/mol
[Assume steam to be an ideal gas. Given \(\Delta_\text{vap}H^{\ominus} \) for water at 373 K and 1 bar is 41.1 kJ mol-1; R=8.31 JK-1 mol-1 ]
1. 38 kJ/mol
2. 42 kJ/mol
3. 35 kJ/mol
4. 33 kJ/mol
Subtopic: Thermochemistry |
52%
Level 3: 35%-60%
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Calculate the standard enthalpy of formation \(\Delta H^0_f\) of \(C_2H_6 \) (in kJ/mole) using the given enthalpy of combustion data:\(\Delta \mathrm{H}^0_{\text {comb. }}\left(\mathrm{C}_{2} \mathrm{H}_{\mathrm{6}}, \mathrm{g}\right)=-1560 \mathrm{~kJ} / \mathrm{mole}\\ \Delta \mathrm{H}^0_{\text {comb. }}(\mathrm{C}, \mathrm{s})=-394 \mathrm{~kJ} / \mathrm{mole}\\ \Delta \mathrm{H}^0_{\text {comb. }}\left(\mathrm{H}_{2}, \mathrm{~g}\right)=-249 \mathrm{~kJ} / \mathrm{mole}\)
| 1. | 25 kJ/mol | 2. | 50 kJ/mol |
| 3. | 1519 kJ/mol | 4. | 1000 kJ/mol |
Subtopic: Thermochemistry |
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Level 2: 60%+
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An ideal gas undergoes isothermal expansion from 4 L to 20 L against vacuum.
Calculate the amount of heat absorbed during the process:
2. –50 kJ
3. 50 kJ
4. –40 kJ
Subtopic: First Law of Thermodynamics |
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Level 1: 80%+
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