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 |
For the 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.
If the Eocell for a given reaction has a negative value, which of the following gives correct relationships for the values of ∆Go and Keq?
1.
2.
3.
4.
A hydrogen gas electrode is made by dipping platinum wire in a solution of HCl of pH = 10 and by passing hydrogen gas around the platinum wire at one atm pressure. The oxidation potential of the electrode would be:
1. | 0.59 V | 2. | 0.118 V |
3. | 1.18 V | 4. | 0.059 V |
The Gibb's energy for the decomposition of \(\mathrm{A l_{2} O_{3}}\) at \(\mathrm{500~ ^\circ C}\) is as follows:
2/3Al2O3 → 4/3Al + O2 ; ∆rG = + 960 k J mol–1
The potential difference needed for the electrolytic reduction of aluminium oxide (Al2O3) at \(\mathrm{500~ ^\circ C}\) is at least,
1. 3.0 V
2. 2.5 V
3. 5.0 V
4. 4.5 V
If the for a given reaction has a negative value, then which of the following gives the correct relationship for the values of ?
1.
2.
3.
4.
Given:
(i) Eo = 0.337 V
(ii) Eo = 0.153 V
Electrode potential, Eo for the reaction,
, will be:
1. 0.52 V
2. 0.90 V
3. 0.30 V
4. 0.38 V