‹ Back to the paper
The standard electrode potential for the reaction is: (I) (II) The will be: The value of standard…
The standard electrode potential for the reaction is:
(I) $\text{Ag}^+ + \text{e}^- \rightarrow \text{Ag}(s); \, E^\circ_{\text{Ag}^+/\text{Ag}} = +0.80\text{ V}$
(II) $\text{Sn}^{2+} + 2\text{e}^- \rightarrow \text{Sn}(s); \, E^\circ_{\text{Sn}^{2+}/\text{Sn}} = -0.14\text{ V}$
(i)
The $E^\circ_{\text{cell}}$ will be:
- (a)0.66 V
- (b)0.88 V
- (c)0.94 V
- (d)1.08 V
(ii)
The value of standard Gibbs energy ($\Delta G^\circ$) will be:
($F = 96,000\text{ C mol}^{-1}$)
- (a)-181.42 kJ
- (b)-90.71 kJ
- (c)-45.36 kJ
- (d)-22.68 kJ
Answer
No answer yet.
From ISC 2022 Specimen Chemistry Paper 1, question 42.