Recent questions and answers in Electrochemistry

For the disproportionation reaction 2Cu+(aq) $\rightleftharpoons$ Cu(s) + Cu2+(aq) at 298 K, In K (where K is the equilibrium constant) is________ 10-1. Given $\left(E_{Cu^{2+}/Cu^+}^o=0.16V,\ E_{Cu^+/Cu}^o=0.52V,\ {RT\over F}=0.025\right)$ Numerical ...

Identify the reaction from following having top position in EMF series (Std. red. potential) according to their electrode potential at 298 K. (1) K+ + 1e– → K(s) (2) Mg2+ + 2e– → Mg(s) (3) Fe2+ + 2e– → Fe(s) (4) Au3+ + 3e– → Au(s)

In a typical fuel cell, the reactant (R) and product (P) are (1) R = H2(g) · N2(g) : P = NH3(aq) (2) R = H2(g) · O2(g) : P = H2O2(l) (3) R = H2(g) · O2(g) : P = H2O(l) (4) R = H2(g) · O2(g) · Cl2(g) : P = HClO4(aq)

The Gibbs energy change (in J) for the given reaction at [Cu2+] = [Sn2+] = 1 M and 298 K is : Cu(s) + Sn2+(aq.) $\longrightarrow$ Cu2+ (aq.) + Sn(s); ($E_{Sn^{2+}|Sn}^0$ = –0.16 V, $E_{Cu^{2+}|Cu}^0$ = 0.34 V, Take F = 96500 C mol–1) Numerical Value Type

In the electrochemical cell : $\require{mhchem}\ce{Zn|ZnSO4}(\text{0.01 M})||\ce{CuSO4}(\text{1.0 M})|\ce{Cu}$, the emf of this Daniell cell is $E_1$. When the concentration of $\ce{ZnSO4}$ is changed to $\text{1.0 M}$ and that of $\ce{CuSO4}$ changed to $\...

The anodic half-cell of lead-acid battery is recharged unsing electricity of 0.05 Faraday. The amount of PbSO4 electrolyzed in g during the process in : (Molar mass of PbSO4 = 303 g mol-1) (1) 22.8 (2) 15.2 (3) 7.6 (4) 11.4

On electrolysis of dil.sulphuric acid using Platinum (Pt) electrode, the product obtained at anode will be: (1) Hydrogen gas (2) Oxygen gas (3) H2S gas (4) SO2 gas

For a cell involving one electron $E^o_{cell}$ = 0.59 V at 298 K, the equilibrium constant for the cell reaction is : $[{\text{Given That } {2.303 RT\over F}=0.059 V\text{ at }T=298K}]$ (1) 1.0 × 102 (2) 1.0 × 105 (3) 1.0 × 1010 (4) 1.0 × 1030

For the cell reaction $2Fe^{3+}(aq) +2I^-(aq)\to 2Fe^{2+} (aq)+ I _2(aq)$ $E^o _{Cell}=0.24 V $ at 298 K. The standard Gibbs energy $(\Delta_r G^o)$ of the cell reaction is : (1) –46.32 kJ mol–1 (2) –23.16 kJ mol–1 (3) 46.32 kJ mol–1 (4) 23.16 kJ mol–1