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Q. No.For an endothermic reaction:
A. \(q_p \) (heat at constant pressure) is negative.
B. \(\Delta _r H \) (enthalpy change of the reaction) is positive.
C. \(\Delta _r H \) is negative.
D. \(q_p \) is positive.
Which of the following combinations is correct?
A. \(q_p \) (heat at constant pressure) is negative.
B. \(\Delta _r H \) (enthalpy change of the reaction) is positive.
C. \(\Delta _r H \) is negative.
D. \(q_p \) is positive.
Which of the following combinations is correct?
| 1. | B and D | 2. | C and D |
| 3. | A and B | 4. | A and C |
Subtopic: Thermodynamics' Properties and process |
73%
Level 2: 60%+
NEET - 2024
Hints
Match List I with List II.
Choose the correct answer from the options given below:
| List-I (Process) | List-II (Conditions) | ||
| A. | Isothermal process | I. | No heat exchange |
| B. | Isochoric process | II. | Carried out at constant temperature |
| C. | Isobaric process | III. | Carried out at constant volume |
| D. | Adiabatic process | IV. | Carried out at constant pressure |
| 1. | \(\text { A-IV, B-II, C-III, D-I }\) | 2. | \(\text { A-I, B-II, C-III, D-IV }\) |
| 3. | \(\text { A-II, B-III, C-IV, D-I }\) | 4. | \(\text { A-IV, B-III, C-II, D-I }\) |
Subtopic: Thermodynamics' Properties and process |
86%
Level 1: 80%+
NEET - 2024
Hints
Consider the following reaction:
\(\mathrm{A}_2(\mathrm{~g})+3 \mathrm{~B}_2(\mathrm{~g}) \rightarrow 2 \mathrm{AB}_3(\mathrm{~g})\)
If at 300K, the enthalpy change for the above reaction is +15 kJ, then the internal energy change is:
\(\mathrm{A}_2(\mathrm{~g})+3 \mathrm{~B}_2(\mathrm{~g}) \rightarrow 2 \mathrm{AB}_3(\mathrm{~g})\)
If at 300K, the enthalpy change for the above reaction is +15 kJ, then the internal energy change is:
| 1. | 19.98 K J | 2. | 200 J |
| 3. | 1999 J | 4. | 1.9988 kJ |
Subtopic: Enthalpy & Internal energy |
76%
Level 2: 60%+
NEET - 2024
Hints
Find the amount of heat released when 35.0 g of CO₂ is formed from the combustion of carbon in dioxygen gas. Given that the enthalpy of combustion of carbon to carbon dioxide is −390.0 kJ mol⁻¹.
| 1. | \(310~\text{kJ}\) | 2. | \(490~\text{kJ}\) |
| 3. | \(245~\text{kJ}\) | 4. | \(700~\text{kJ}\) |
Subtopic: Enthalpy & Internal energy |
74%
Level 2: 60%+
NEET - 2024
Hints
What is the correct relationship between changes in enthalpy and internal energy within the following options?
1. \(\mathrm{\Delta {H}+\Delta {U}=\Delta {nR}} \)
2. \(\mathrm{\Delta {H}=\Delta {U -\Delta n_gRT}}\)
3. \(\mathrm{\Delta {H}=\Delta {U+\Delta n_gRT }}\)
4. \(\mathrm{\Delta {H} -\Delta {U=-\Delta n_gRT}}\)
1. \(\mathrm{\Delta {H}+\Delta {U}=\Delta {nR}} \)
2. \(\mathrm{\Delta {H}=\Delta {U -\Delta n_gRT}}\)
3. \(\mathrm{\Delta {H}=\Delta {U+\Delta n_gRT }}\)
4. \(\mathrm{\Delta {H} -\Delta {U=-\Delta n_gRT}}\)
Subtopic: Enthalpy & Internal energy |
83%
Level 1: 80%+
NEET - 2023
Hints
For the reaction, 2Cl(g) Cl2(g), the correct option is:
| 1. | \(\Delta_{\mathrm{r}} \mathrm{H}>0\) and \(\Delta_{\mathrm{r}} \mathrm{S}<0 \) | 2. | \(\Delta_{\mathrm{r}} \mathrm{H}<0\) and \( \Delta_{\mathrm{r}} \mathrm{S}>0 \) |
| 3. | \(\Delta_{\mathrm{r}} \mathrm{H}<0 \) and \(\Delta_{\mathrm{r}} \mathrm{S}<0 \) | 4. | \(\Delta_{\mathrm{r}} \mathrm{H}>0\) and \( \Delta_{\mathrm{r}} \mathrm{S}>0\) |
Subtopic: Enthalpy & Internal energy | Spontaneity & Entropy |
61%
Level 2: 60%+
NEET - 2020
Hints
The standard enthalpy of vaporization for water at 100 oC is 40.66 kJ mol–1. The internal energy of vaporization of water at 100 oC (in kJ mol–1) is:
(Assume water vapour behaves like an ideal gas.)
| 1. | +37.56 | 2. | –43.76 |
| 3. | +43.76 | 4. | +40.66 |
Subtopic: Enthalpy & Internal energy |
61%
Level 2: 60%+
AIPMT - 2012
Hints
Which of the following options correctly represents the relationship between \(C_p \text { and } C_V\) for one mole of an ideal gas?
| 1. | \(C_P=R C_V \) | 2. | \(C_V=RC_P \) |
| 3. | \(C_P+C_V=R \) | 4. | \(C_{{P}}-{C}_{{V}}={R}\) |
Subtopic: Cp & Cv |
88%
Level 1: 80%+
NEET - 2021
Hints
Choose the correct statement for the work done in the expansion and heat absorbed or released when 5 liters of an ideal gas at 10 atmospheric pressure isothermally expands into a vacuum until the volume is 15 liters:
| 1. | Both the heat and work done will be greater than zero. |
| 2. | Heat absorbed will be less than zero and work done will be positive. |
| 3. | Work done will be zero and heat absorbed or evolved will also be zero. |
| 4. | Work done will be greater than zero and heat absorbed will remain zero. |
Subtopic: First Law of Thermodynamics |
62%
Level 2: 60%+
NEET - 2024
Hints
Work done during reversible isothermal expansion of one mole of hydrogen gas at 25°C from a pressure of 20 atmospheres to a pressure of 10 atmospheres is:
(Given: R = 2.0 cal K–1 mol–1)
(Given: R = 2.0 cal K–1 mol–1)
| 1. | –413.14 calories | 2. | 413.14 calories |
| 3. | 100 calories | 4. | 0 calorie |
Subtopic: First Law of Thermodynamics |
70%
Level 2: 60%+
NEET - 2024
Hints
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