Electrochemistry Quiz-1

Given that the dissociation content of acetic is $1.8 \times 10^{-5}$ and its molar conductivity at infinite dilution is $390.7\,\Omega^{-1}{\text{cm}^{-2}\text{mol}^{-1}}$ . The molar conductivity of 0.01 M acetic acid solution will be

The standard electrode potential ($E^\circ$) for $OCl^-/Cl^-$ and $Cl^-/\frac12Cl_2$ respectively are 0.94 V and - 1.36 V. The $E^\circ$ value for $OCl^-/\frac12Cl_2$ will be

The standard electrode potentials for $Zn^{2+}/Zn, Ni^{2+}/ Ni,$ and $Fe^{2+}/ Fe$ are -0.76, -0.23, and -0.44 V respectively. The reaction $X + Y^{2+}\longrightarrow X^{2+}+Y$ will be spontaneous when:

$E^\circ_{cell}$ for the reaction, $Fe + Zn^{2+}\rightleftharpoons Fe^{2+}+ Zn$ is -0.32 V. The equilibrium concentration of $Fe^{2+}$ when a piece of iron is placed in 1 M $Zn^{2+}$solution is

A solution contains $Fe^{2+},Fe^{3+}$ and $I^-$ ions. This solution was treated with iodine at $35^\circ C$. $E^\circ$ for $Fe^{3+}/ Fe^{2+}$is + 0.77 V and for $I_2 / 2I^-$ is 0.536 V. The favourable redox reaction is

If $Zn^{+2}/Zn$ electrode is diluted 100 times, then the change in emf is

The standard reduction potential values of the three metallic cation X, Y and Z are 0.52, -3.03 and -1.18 V respectively. The order of reducing power of the corresponding metals is

A gas Y at 1 bar is bubbled through a solution containing a mixture of 1M X and 1M Z at $25^\circ C$. If the reduction potential of Z > Y > X, then

For the electrochemical cell, $M | M^+ || X^- | X, E^\circ_{M^+|M} = 0.44\,V$ and $E^\circ_{X|X^-}=0.33\,V$. From this data one can deduct that

The value of $E_{H_2O|H_2(1bar)|Pt}$ at 298 would be