- 1(current)
Q. No.Consider the following reaction:
2A (g) + B (g) → 2D (g)
\(ΔU^⊖\)=−10 \(kJ mol^{−1}\) and \(ΔS^⊖\)=−44 \(J K^{−1}\) at 298 K.
Identify the correct option with \(ΔG^⊖\) for the reaction and spontaneity of the reaction at 298 K.
(Given : R=\(8.31 ~J mol^{−1} K^{−1}\))
2A (g) + B (g) → 2D (g)
\(ΔU^⊖\)=−10 \(kJ mol^{−1}\) and \(ΔS^⊖\)=−44 \(J K^{−1}\) at 298 K.
Identify the correct option with \(ΔG^⊖\) for the reaction and spontaneity of the reaction at 298 K.
(Given : R=\(8.31 ~J mol^{−1} K^{−1}\))
| 1. | −1.635 kJ mol−1, spontaneous |
| 2. | +0.63568 kJ mol−1, non-spontaneous |
| 3. | −0.63568 kJ mol−1, spontaneous |
| 4. | +1.635 kJ mol−1, non-spontaneous |
Subtopic: Spontaneity & Entropy | Gibbs Energy Change |
56%
Level 3: 35%-60%
NEET - 2026
Please attempt this question first.
Hints
Please attempt this question first.
Two moles of an ideal gas undergo free expansion from 10 L to 100 L at 300 K. The Values of \(\Delta \mathrm{S}_{\text {system }}\) and \(\Delta \mathrm{S}_{\text {surroundings }}\) are :
(R is universal gas constant)
(R is universal gas constant)
| 1. | \(\Delta \mathrm{S}_{\text {system }}=4.606 \mathrm~{R} ; \Delta \mathrm{S}_{\text {surroundings }}=0\) |
| 2. | \(\Delta \mathrm{~S}_{\text {system }}=0 ;~ \Delta \mathrm{S}_{\text {surroundings }}=0 \) |
| 3. | \(\Delta \mathrm{~S}_{\text {system }}=4.606~ \mathrm{R} ; \Delta \mathrm{S}_{\text {surroundings }}= -4.606 \mathrm{R}\) |
| 4. | \(\Delta \mathrm{~S}_{\text {system }}=0 ; \quad \Delta ~~\mathrm{S}_{\text {surroundings }}= 4.606 \mathrm{R}\) |
Subtopic: Spontaneity & Entropy |
Level 4: Below 35%
NEET - 2026
Please attempt this question first.
Hints
Please attempt this question first.
In which of the following processes entropy increases?
Choose the correct answer from the options given below:
| A. | A liquid evaporates to vapour. |
| B. | Temperature of a crystalline solid lowered from \(130~\text{K}\) to \(0~\text{K}.\) |
| C. | \(2 \mathrm{NaHCO}_{3(\mathrm{~s})} \rightarrow \mathrm{Na}_2 \mathrm{CO}_{3(\mathrm{~s})}+\mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}\) |
| D. | \(\mathrm{Cl}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{Cl}_{(\mathrm{g})}\) |
| 1. | \(\text { A, B and D }\) | 2. | \(\text { A, C and D }\) |
| 3. | \(\text { C and D }\) | 4. | \(\text { A and C }\) |
Subtopic: Spontaneity & Entropy |
73%
Level 2: 60%+
NEET - 2024
Hints
Which of the following statements is correct for an irreversible isothermal expansion of an ideal gas?
1.
2.
3.
4.
Subtopic: Spontaneity & Entropy |
69%
Level 2: 60%+
NEET - 2021
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
If for a certain reaction is 30 kJ mol–1 at 450 K, the value of (in JK–1 mol–1) for which the same reaction will be spontaneous at the same temperature is:
| 1. | 70 | 2. | –33 |
| 3. | 33 | 4. | –70 |
Subtopic: Spontaneity & Entropy |
71%
Level 2: 60%+
NEET - 2020
Hints
- 1(current)
Q. No.
© 2026 GoodEd Technologies Pvt. Ltd.