List of top Chemistry Questions on Galvanic Cells

Which of the following reactions correctly represents a Daniell Cell?
If one faraday of electricity is used in the discharging of \(Cu^{2+}\), then find the mass (ing) of \(Cu\) deposited (nearest integer)
At what \(pH\), given half cell \(MnO _4^{-}(01 M ) \mid Mn ^{2+}(0001 M )\) will have electrode potential of \(1.282\, V\)? (Nearest Integer)
(Given: \(E _{ MnO _{4}^-| Mn ^{2+}}^{ o }=154 \,V , \frac{2303 RT }{ F }=0059\, V\))

\(Pt(s) ∣ H2​(g)(1atm) ∣ H+(aq, [H+]=1)\, ∥\, Fe3+(aq), Fe2+(aq) ∣ Pt(s)\)
Given\( E^∘_{Fe^{3+}Fe^{2+}}\)\(=0.771V\) and \(E^∘_{H^{+1/2}H_2}​=0\,V,T=298K\)
If the potential of the cell is 0.712V, the ratio of concentration of \(Fe2+\) to \(Fe3+\) is

In a cell, the following reactions take place
\(Fe^{2+} → Fe^{3+} + e^-\)
\(E°_{Fe^{3+}/Fe^{2+}} = 0.77\ V\)
\(2I^- → I_2 + 2e^-\)
\(E_{I_2/I^-} = 0.54\ V\)
The standard electrode potential for the spontaneous reaction in the cell is \(x×10^{–2} V\) at \(208\ K\). The value of \(x\) is _______. (Nearest Integer)
For a cell, \(Cu(s)|Cu^{2+}(0.001M)||Ag^+(0.01M)|Ag(s)\)
the cell potential is found to be \(0.43 V\) at \(298 K\). The magnitude of standard electrode potential for \(Cu^{2+}/{Cu}\) is ____ \(× 10^{–2}\) V.
[Given: \(E_{Ag^+/Ag^⊖}=0.80\) V and \(\frac {2.303RT}{F}=0.06 V\)]
In the cell ${Pt(s) | H_2(g , 1 bar | HCl(aq) | Ag(s) | Pt(s)} $ the cell potential is 0.92 when a $10^{-6}$ molal HCl solution is used. THe standard electrode potential of ${(AgCl/Ag,Cl^{-})}$ electrode is : $\left\{ \text{given} , \frac{2.303RT}{F} = 0.06 V \; at \; 298K\right\}$