1. | \(-61.75 \mathrm{{~kJ} {~mol}}^{-1}\) | 2. | \(+5.006 \mathrm{{~kJ} {~mol}}^{-1}\) |
3. | \(-5.006 \mathrm{{~kJ} {~mol}}^{-1}\) | 4. | \(+61.75 \mathrm{{~kJ} {~mol}}^{-1}\) |
Assertion (A): | \(\Delta_{\mathrm{r}} \mathrm{G}=-\mathrm{nFE} _{\text {cell }}, \) value \(\mathrm{\Delta_rG }\) depends on n. | In equation
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. |
1. | –200.27 kJ mol–1 | 2. | –212.27 kJ mol–1 |
3. | –212.27 J mol–1 | 4. | –200.27 J mol–1 |
Given the following cell reaction:
\(\mathrm{2Fe^{3+}(aq) \ + \ 2I^{-}(aq)\rightarrow 2Fe^{2+}(aq) \ + \ I_{2}(aq)}\)
\(E_{cell}^{o} \ = \ 0.24 \ V\) at .
The standard Gibbs energy ∆rG⊝ of the cell reaction is:
[Given: ]
1.
2.
3.
4.
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. | 2. | ||
3. | 4. |
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