List of top Chemistry Questions on Standard electrode potentials and electrochemical cells

The standard electrode potential (\(E^\circ\)) for the half-cell reaction \(\text{Fe}^{3+} + e^- \rightarrow \text{Fe}^{2+}\) at \(298\text{ K}\) is (Given: \(E^\circ(\text{Fe}^{3+}/\text{Fe}) = -0.04\text{ V}\) and \(E^\circ(\text{Fe}^{2+}/\text{Fe}) = -0.44\text{ V}\) at \(298\text{ K}\))
Standard electrode potentials (\(\mathrm{M^{n+}/M}\)) of four metals A, B, C and D are given below: (A) \(-1.2\text{ V}\) (B) \(+0.5\text{ V}\) (C) \(+1.2\text{ V}\) (D) \(-3.0\text{ V}\) The correct increasing order for the reducing power of these metals will be:
The oxidation potentials of \(A\) and \(B\) are \[ +2.37\ \mathrm{V} \quad \text{and} \quad +1.66\ \mathrm{V} \] respectively. In chemical reactions
The oxidation potentials of A and B are +2.37 V and +1.66 V respectively. In chemical reactions
The oxidation potentials of A and B are +2.37 V and +1.66 V respectively. In chemical reactions
The oxidation potentials of A and B are +2.37 V and +1.66 V respectively. In chemical reactions
The oxidation potentials of A and B are +2.37 V and +1.66 V respectively. In chemical reactions
Ecell for the given cell pt(s)/Br2(1)/Br-(0.1 M)//Cl-(0.01 M)/Cl2(g) (1 atm)/Pt(s) [Given Ebr2/Br-=+1.09 V,E Cl2/Cl-=1.36 V] at 298 K is
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 electrode would be