Tamil Nadu Board Solutions for Chapter: Electro Chemistry, Exercise 1: EVALUATION

Calculate the molar conductance of $0.01 \mathrm{M}$ aqueous $\mathrm{KCl}$ solution at $25°\mathrm{C}$. The specific conductance of $\mathrm{KCl}$ at $25°\mathrm{C}$ is $14.114 \times {10}^{-2} {\mathrm{Sm}}^{-1}$ .

The resistance of a $0.15 \mathrm{N}$ solution of an electrolyte is $50 \mathrm{\Omega }$. The specific conductance of a solution is $2.4 {\mathrm{Sm}}^{-1}$. The resistance of $0.5 \mathrm{N}$ solution of same electrolyte measured using the same conductivity cell is $480 \mathrm{\Omega }$. Find the equivalent conductivity of $0.5 \mathrm{N}$ solution of the electrolyte.

The emf of the following cell at $25°\mathrm{C}$ is equal to $0.34 \mathrm{V}$. Calculate the reduction potential of copper electrode.
$\mathrm{Pt} \left(\mathrm{s}\right)\overline{){\mathrm{H}}_2 (\mathrm{g}, 1 \mathrm{atm})} \overline{)\mathrm{H} (\mathrm{aq}, 1\mathrm{M})}\parallel {\mathrm{Cu}}^{2+}(\mathrm{aq}, 1 \mathrm{M}) \overline{)\mathrm{Cu} \left(\mathrm{s}\right)}$

Using the calculated emf value of zinc and copper electrode, calculate the emf of the following cell at $25°\mathrm{C}$.

$\mathrm{Zn} \left(\mathrm{s}\right) \overline{){\mathrm{Zn}}^{2+} (\mathrm{aq}, 1 \mathrm{M})}\parallel {\mathrm{Cu}}^{2+}(\mathrm{aq}, 1 \mathrm{M}) \overline{)\mathrm{Cu} \left(\mathrm{s}\right)}$

Write the overall redox reaction which takes place in the galvanic cell,

$\mathrm{Pt}\left(\mathrm{s}\right)\mid {\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right), {\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right)\parallel {\mathrm{MnO}}_4^{-}\left(\mathrm{aq}\right), {\mathrm{H}}^{+}\left(\mathrm{aq}\right), {\mathrm{Mn}}^{2+}\left(\mathrm{aq}\right)\mid \mathrm{Pt}\left(\mathrm{s}\right)$

The electrochemical cell reaction of the Daniel cell is
$\mathrm{Zn} \left(\mathrm{s}\right) + {\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right) \to {\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)+\mathrm{Cu} \left(\mathrm{s}\right)$

What is the change in the cell voltage on increasing the ion concentration in the anode compartment by a factor $10$?

A solution of a salt of metal was electrolysed for $15$ minutes with a current of $0.15$ amperes. The mass of the metal deposited at the cathode is $0.783 \mathrm{g}$. Calculate the equivalent mass of the metal.

Ionic conductance at infinite dilution of ${\mathrm{Al}}^{3+}$ and ${\mathrm{SO}}_4{ }^{2-}$are $189$ and $160$ $\mathrm{mho} {\mathrm{cm}}^2 {\mathrm{equiv}}^{-1}$. Calculate the equivalent and molar conductance of the electrolyte ${\mathrm{Al}}_2({\mathrm{SO}}_4{)}_3$ at infinite dilution.