If the emf of the cell Cu(s) | Cu^{2+}(1 text | vedclass

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Question

(C) The standard cell potential $E^0_{cell}$ is given by the difference between the standard reduction potentials of the cathode and the anode:$E^0_{c

Vedclass · Accepted Answer

$0.8$

Vedclass · Answer

(C) The standard cell potential $E^0_{cell}$ is given by the difference between the standard reduction potentials of the cathode and the anode:$E^0_{cell} = E^0_{cathode} - E^0_{anode}$Here, the cathode is $Ag$ and the anode is $Cu$, so:$E^0_{cell} = E^0_{Ag^+/Ag} - E^0_{Cu^{2+}/Cu}$Given $E^0_{cell} = 0.463 	ext{ V}$ and $E^0_{Cu^{2+}/Cu} = 0.337 	ext{ V}$:$0.463 	ext{ V} = E^0_{Ag^+/Ag} - 0.337 	ext{ V}$$E^0_{Ag^+/Ag} = 0.463 	ext{ V} + 0.337 	ext{ V} = 0.800 	ext{ V}$Thus, the standard potential of the $Ag$ electrode is $0.8 	ext{ V}$.

If the $emf$ of the cell $Cu(s) | Cu^{2+}(1 \text{ M}) || Ag^+(1 \text{ M}) | Ag(s)$ is $0.463 \text{ V}$ at $25^{\circ} \text{C}$ and the standard electrode potential of the $Cu$ electrode is $0.337 \text{ V}$, find the standard electrode potential of the $Ag$ electrode. (in $\text{ V}$)

Similar Questions

Given,for $Sn^{4+} / Sn^{2+}$,standard reduction potential is $0.15 \ V$ and for $Au^{3+} / Au$,standard reduction potential is $1.5 \ V$. For the reaction,$3 Sn^{2+} + 2 Au^{3+} \longrightarrow 3 Sn^{4+} + 2 Au$,the value of $E_{\text{cell}}^{\circ}$ is:

Which of the following is the weakest reducing agent?

In a cell reaction
$Cu_{(s)} + 2Ag^{+}_{(aq)} \to Cu^{2+}_{(aq)} + 2Ag_{(s)}$
$E_{cell}^o = + 0.46 \ V$.
If the concentration of $Cu^{2+}$ ions is doubled,then $E_{cell}^o$ will be

$A$ standard hydrogen electrode has zero electrode potential because

Given $:$
$(i) \, Cu^{2+} + 2e^- \rightarrow Cu \,, \, E^o = 0.337 \, V$
$(ii) \, Cu^{2+} + e^- \rightarrow Cu^{+} \,, \, E^o = 0.153 \, V$
Electrode potential,$E^o$ for the reaction,
$Cu^{+} + e^- \rightarrow Cu \,,$ will be $............$ $V$.

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