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Q. No.Given below are two statements:
Assertion (A):
Pressure is an intensive property.
Reason (R):
Volume is an extensive property.
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: Classification of System, Extensive & Intensive Properties |
81%
Level 1: 80%+
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Given below are two statements:
| Assertion (A): | Variables like P, V, and T are called state functions. |
| Reason (R): |
Their values depend solely on the system's state, and not on how it is reached. |
| 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: Thermodynamics' Properties and process |
85%
Level 1: 80%+
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Which reaction has ΔH∘reaction equal to the \(\Delta H_f^{\circ}\) of CaSO3(s)?
1. Ca(s) + \(\frac{1}{8}\) S8(s, rhombic) + \(\frac{3}{2}\) O2(g) → CaSO3(s)
2. 8Ca(s) + S8(s) + 12O2(g) → 8CaSO3(s)
3. 8Ca(s) + S8(g) + 12O2(g) → 8CaSO3(s)
4. CaO(s) + SO2(g) → CaSO3(s)
1. Ca(s) + \(\frac{1}{8}\) S8(s, rhombic) + \(\frac{3}{2}\) O2(g) → CaSO3(s)
2. 8Ca(s) + S8(s) + 12O2(g) → 8CaSO3(s)
3. 8Ca(s) + S8(g) + 12O2(g) → 8CaSO3(s)
4. CaO(s) + SO2(g) → CaSO3(s)
Subtopic: Thermochemistry |
79%
Level 2: 60%+
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Burning 48.0 g of graphite in excess oxygen under standard conditions releases 1574.0 kJ of heat. What is \(\Delta H_f^{\circ}\) of CO2(g)?
1. 157 kJ mol-1
2. –1574 kJ mol-1
3. –394 kJ mol-1
4. 32.8 kJ mol-1
1. 157 kJ mol-1
2. –1574 kJ mol-1
3. –394 kJ mol-1
4. 32.8 kJ mol-1
Subtopic: Thermochemistry |
71%
Level 2: 60%+
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Given the standard enthalpies of the gas-phase reactions of hydrogen sulphide, what is the standard enthalpy of reaction for the gas-phase combustion of carbon disulphide?
1. –450.4 kJ mol–1
2. –586.0 kJ mol–1
3. –968.6 kJ mol–1
4. –1104.2 kJ mol–1
| Reaction | Δ Hºrxn, kJ mol–1 |
| H2S + 1.5O2 → SO2 + H2O | –518.2 |
| 2H2S + CO2 → CS2 + 2H2O | 67.8 |
| CS2 + 3O2 → CO2 + 2SO2 | ??? |
2. –586.0 kJ mol–1
3. –968.6 kJ mol–1
4. –1104.2 kJ mol–1
Subtopic: Hess's Law |
74%
Level 2: 60%+
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For the given cycle, the work done during the isobaric process is:
| 1. | \(200\) J | 2. | zero |
| 3. | \(400\) J | 4. | \(600\) J |
Subtopic: Work Done by a Gas |
57%
Level 3: 35%-60%
NEET - 2023
Hints
Which of the following relations does not give the equation of an adiabatic process, where terms have their usual meaning?
1. \({P}^{1-\gamma}{T}^{\gamma}= \text{constant}\)
2. \({PV}^{\gamma}=\text{constant}\)
3. \({TV}^{\gamma-1}= \text{constant}\)
4. \({P}^{\gamma} {T}^{1-\gamma}=\text{constant}\)
1. \({P}^{1-\gamma}{T}^{\gamma}= \text{constant}\)
2. \({PV}^{\gamma}=\text{constant}\)
3. \({TV}^{\gamma-1}= \text{constant}\)
4. \({P}^{\gamma} {T}^{1-\gamma}=\text{constant}\)
Subtopic: Types of Processes |
76%
Level 2: 60%+
NEET - 2013
Hints
A system is taken from state \(a\) to state \(c\) by two paths \(adc\) and \(abc\) as shown in the figure. The internal energy at \(a\) is \({U}_{a}=10~\text{J}.\) Along the path \(adc\) the amount of heat absorbed \(\delta Q_1=50~\text{J}\) and the work obtained \(\delta W_1=20~\text{J}\) whereas along the path \(abc\) the heat absorbed \(\delta Q_2 = 36~\text{J}.\) The amount of work along the path \(abc\) is:
| 1. | \(10~\text{J}\) | 2. | \(12~\text{J}\) |
| 3. | \(36~\text{J}\) | 4. | \(6~\text{J}\) |
Subtopic: First Law of Thermodynamics |
79%
Level 2: 60%+
NEET - 2013
Hints
1 mol of monoatomic ideal gas expanded adiabatically against a constant pressure of 2 atm from 10L to 20L. The correct option for the above process is:
1. q = 20 L-atm
2. \(\Delta U = 0 \)
3. \(\Delta U = -20 ~\text L~\text {atm} \)
4. \(\text w = 10 ~\text L~ \text {atm} \)
1. q = 20 L-atm
2. \(\Delta U = 0 \)
3. \(\Delta U = -20 ~\text L~\text {atm} \)
4. \(\text w = 10 ~\text L~ \text {atm} \)
Subtopic: First Law of Thermodynamics |
82%
Level 1: 80%+
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| Statement I: | ∆S total i.e., ∆Ssys + ∆Ssurr is zero for the irreversible process. |
| Statement II: | Total entropy change for the system and surrounding of a spontaneous process is zero. |
| 1. | Statement I is False but Statement II is True. |
| 2. | Both Statement I and Statement II are True. |
| 3. | Both Statement I and Statement II are False. |
| 4. | Statement I is True but Statement II is False. |
Subtopic: Spontaneity & Entropy |
54%
Level 3: 35%-60%
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