Academic Experts Solutions for Chapter: Electrochemistry, Exercise 1: Exercise

The conductivity of a saturated solution of ${\mathrm{BaSO}}_4$ is $3.06\times {10}^{-6} {\mathrm{ohm}}^{-1} {\mathrm{cm}}^{-1}$ and its equivalent conductance is $1.53 {\mathrm{ohm}}^{-1} {\mathrm{cm}}^2 {\mathrm{equiv}}^{-1}$. The ${\mathrm{K}}_{\mathrm{sp}}$ for ${\mathrm{BaSO}}_4$ will be:

Consider the reaction: $\left(\mathrm{T}=298 \mathrm{K}\right)$

${\mathrm{Cl}}_2\left(\mathrm{g}\right)+2{\mathrm{Br}}^{-}\left(\mathrm{aq}\right)⟶2{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)+{\mathrm{Br}}_2\left(\mathrm{aq}\right)$

Determine the emf (in volts) of the cell, when $\left[{\mathrm{Cl}}^{-}\right]=\left[{\mathrm{Br}}_2\right]=\left[{\mathrm{Br}}^{-}\right]=0.01 \mathrm{M}$ and ${\mathrm{Cl}}_2$ gas is at $1 \mathrm{atm}$ pressure.

($\mathrm{E}°$ for the above reaction is $=0.29$ volt)

Enter only the numerical value in the box  and exclude the units.

$\mathrm{Zn}+{\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)\rightleftharpoons \mathrm{Cu}+{\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)$

Reaction quotient is $\mathrm{Q}=\frac{\left[{\mathrm{Zn}}^{2+}\right]}{\left[{\mathrm{Cu}}^{2+}\right]}$. $\mathrm{E}{°}_{\mathrm{cell}}=1.10 \mathrm{V}$. ${\mathrm{E}}_{\mathrm{cell}}$ will be $1.1591 \mathrm{V}$. The value of  $\frac{\left[{\mathrm{Zn}}^{2+}\right]}{\left[{\mathrm{Cu}}^{2+}\right]}$ is ${10}^{-\mathrm{x}}$, the value of $\mathrm{x}$ is

Round off your answer to the nearest integer.

Four moles of electrons were transferred from anode to cathode in an experiment on the electrolysis of water. Determine the total volume of the two gases (dry and at $\mathrm{STP}$) produced: (in litres).

A cell $\mathrm{Cu}\left|{\mathrm{Cu}}^{++}\Vert {\mathrm{Ag}}^{+}\right|\mathrm{Ag}$, initially contains $2 \mathrm{M} {\mathrm{Ag}}^{+}$ and $2 \mathrm{M} {\mathrm{Cu}}^{++}$ ions in $1 \mathrm{L}$ electrolyte. Determine the change in cell potential after the passage of $10 \mathrm{amp}$ current for $4825 \sec$.

The half cell reactions for rusting of iron are:
$2{\mathrm{H}}^{+}+\frac{1}{2}{\mathrm{O}}_2+2{\mathrm{e}}^{-}⟶{\mathrm{H}}_2\mathrm{O}; \mathrm{E}°=+1.23 \mathrm{V}, {\mathrm{Fe}}^{2+}+2{\mathrm{e}}^{-}⟶\mathrm{Fe}; \mathrm{E}°=-0.44 \mathrm{V}$
Determine $\mathrm{\Delta G}°$ (in $\mathrm{kJ}$) for the reaction.

The limiting molar conductivities $\mathrm{\Lambda }°$ for $\mathrm{NaCl}, \mathrm{KBr}$ and $\mathrm{KCl}$ are $126, 152$ and $150 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$ respectively. Determine the $\mathrm{\Lambda }°$ for $\mathrm{NaBr}$.

Aluminium oxide may be electrolysed at $1000{}^{\circ }\mathrm{C}$ to furnish the aluminium metal (At. Mass $=27 \mathrm{amu}$; $1$ Faraday $=96,500$ Coulombs). The cathode reaction is ${\mathrm{Al}}^{3+}+3{\mathrm{e}}^{-}\to {\mathrm{Al}}^{}$. To prepare $5.12 \mathrm{kg}$ of aluminium metal by this method, If $5.49\times {10}^{\mathrm{y}} \mathrm{C}$ electricity would be required. then value of y will be.