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.

In the light of the above statements choose the correct answer from the options given below:

 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 |
57%
From NCERT
NEET - 2023
Please attempt this question first.
Hints
Please attempt this question first.

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)
 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 |
80%
From NCERT
NEET - 2022
To view explanation, please take trial in the course.
NEET 2023 - Target Batch - Aryan Raj Singh
Hints
To view explanation, please take trial in the course.
NEET 2023 - Target Batch - Aryan Raj Singh

For the cell reaction
$$\mathrm{2Fe^{3+}(aq) \ + \ 2I^{-}(aq)\rightarrow 2Fe^{2+}(aq) \ + \ I_{2}(aq)}$$

$$E_{cell}^{o} \ = \ 0.24 \ V$$ at $298$ $\mathrm{K}$. The standard Gibbs energy ∆rG of the cell reaction is:

[Given:  $\mathrm{C}$ ${\mathrm{mol}}^{-1}$]

1. $23.16$ $\mathrm{kJ}$ ${\mathrm{mol}}^{-1}$

2. $-46.32$ $\mathrm{kJ}$ ${\mathrm{mol}}^{-1}$

3. $-23.16$ $\mathrm{kJ}$ ${\mathrm{mol}}^{-1}$

4. $46.32$ $\mathrm{kJ}$ ${\mathrm{mol}}^{-1}$

Subtopic:  Relation between Emf, G, Kc & pH |
74%
From NCERT
NEET - 2019
To view explanation, please take trial in the course.
NEET 2023 - Target Batch - Aryan Raj Singh
Hints
To view explanation, please take trial in the course.
NEET 2023 - Target Batch - Aryan Raj Singh

For a cell involving one electron  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. $1.0×{10}^{30}$

2. $1.0×{10}^{2}$

3. $1.0×{10}^{5}$

4. $1.0×{10}^{10}$

Subtopic:  Relation between Emf, G, Kc & pH |
69%
From NCERT
NEET - 2019
To view explanation, please take trial in the course.
NEET 2023 - Target Batch - Aryan Raj Singh
Hints