- 1(current)
Q. No.The standard cell potential of the following cell \(\mathrm{{Zn}\left|{Zn}^{2+}({aq}) \| {Fe}^{2+}({aq})\right| {Fe}~\text{ is }~0.32 {~V}}.\) Calculate the standard Gibbs energy change for the reaction:
\(\mathrm{{Zn}({s})+{Fe}^{2+}({aq}) \rightarrow {Zn}^{2+}({aq})+{Fe}({s})}\)
(Given : \(1 \mathrm{~F}=96487 \mathrm{C} mol^{-1}\))
\(\mathrm{{Zn}({s})+{Fe}^{2+}({aq}) \rightarrow {Zn}^{2+}({aq})+{Fe}({s})}\)
(Given : \(1 \mathrm{~F}=96487 \mathrm{C} mol^{-1}\))
| 1. | \(-61.75 \mathrm{{~kJ} {~mol}}^{-1}\) | 2. | \(+5.006 \mathrm{{~kJ} {~mol}}^{-1}\) |
| 3. | \(-5.006 \mathrm{{~kJ} {~mol}}^{-1}\) | 4. | \(+61.75 \mathrm{{~kJ} {~mol}}^{-1}\) |
Subtopic: Relation between Emf, G, Kc & pH |
84%
Level 1: 80%+
NEET - 2024
Hints
Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R):
| Assertion (A): | In equation \(\Delta_{\mathrm{r}} \mathrm{G}=-\mathrm{nFE} _{\text {cell }}, \) value \(\mathrm{\Delta_rG }\) depends on n. |
| Reason (R): | \(\mathrm{E_{cell} }\) is an intensive property and \(\mathrm{\Delta_rG }\) is an extensive property. |
| 1. | (A) is False but (R) is True. |
| 2. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
| 3. | Both (A) and (R) are True and (R) is not the correct explanation of (A). |
| 4. | (A) is True but (R) is False. |
Subtopic: Relation between Emf, G, Kc & pH |
59%
Level 3: 35%-60%
NEET - 2023
Hints
Standard electrode potential for the cell with cell reaction
Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)
is 1.1 V. Calculate the standard Gibbs energy change for the cell reaction. (Given F = 96487 C mol–1)
Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)
is 1.1 V. Calculate the standard Gibbs energy change for the cell reaction. (Given F = 96487 C mol–1)
| 1. | –200.27 kJ mol–1 | 2. | –212.27 kJ mol–1 |
| 3. | –212.27 J mol–1 | 4. | –200.27 J mol–1 |
Subtopic: Relation between Emf, G, Kc & pH |
82%
Level 1: 80%+
NEET - 2022
Hints
Given the following cell reaction:
\(\mathrm{2Fe^{3+}(aq) \ + \ 2I^{-}(aq)\rightarrow 2Fe^{2+}(aq) \ + \ I_{2}(aq)}\)
The standard Gibbs energy ∆rG⊝ of the cell reaction is:
[Given: \(F = 96500\) \(C\) \(mol^{- 1}\)]
1. \(23 . 16\) \(kJ\) \(mol^{- 1}\)
2. \(- 46 . 32\) \(kJ\) \(mol^{- 1}\)
3. \(- 23 . 16\) \(kJ\) \(mol^{- 1}\)
4. \(46 . 32\) \(kJ\) \(mol^{- 1}\)
Subtopic: Relation between Emf, G, Kc & pH |
75%
Level 2: 60%+
NEET - 2019
Hints
For a cell involving one electron \(E_{cell}^{\ominus} = 0 . 59 V\) at 298 K. The equilibrium constant for the cell reaction is :
\(\mathrm{[Given~ that~ \frac {2.303 ~RT}{F} = 0.059 ~V~ at~ T = 298 K]}\)
| 1. | \(1 . 0 \times \left(10\right)^{30}\) | 2. | \(1 . 0 \times \left(10\right)^{2}\) |
| 3. | \(1 . 0 \times \left(10\right)^{5}\) | 4. | \(1 . 0 \times \left(10\right)^{10}\)
|
Subtopic: Relation between Emf, G, Kc & pH |
73%
Level 2: 60%+
NEET - 2019
Hints
Links
- 1(current)
Q. No.
© 2025 GoodEd Technologies Pvt. Ltd.