Embibe Experts Solutions for Chapter: Electrochemistry, Exercise 1: EXERCISE-1

The reduction potential of a hydrogen electrode at $\mathrm{pH}10$ at $298 \mathrm{K}$ is : $(\mathrm{p}=1 \mathrm{atm})$

A chemist wants to produce ${\mathrm{Cl}}_2\left(\mathrm{g}\right)$ from molten $\mathrm{NaCl}.$ How many grams could be produced if he uses a steady current of $2$ ampere for $2.5$ minutes :-

$\mathrm{Fe}$ Can displace which of the following ions from their aqueous solutions?

(a) ${\mathrm{Na}}^{+}$

(b) ${\mathrm{Zn}}^{2+}$

(c) ${\mathrm{Cu}}^{2+}$

(d) ${\mathrm{Ag}}^{+}$

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.

In an electrochemical cell that function as a voltaic cell :-

The conductivity of a saturated solution of ${\mathrm{Ag}}_3{\mathrm{PO}}_4$ is $9\times {10}^{-6} \mathrm{S}{ \mathrm{m}}^{-1}$ and its equivalent conductivity is $1.50\times {10}^{-4} \mathrm{S}{ \mathrm{m}}^2$ equivalent${}^{-1}.$ The ${\mathrm{K}}_{\mathrm{sp}}$ of ${\mathrm{Ag}}_3{\mathrm{PO}}_4$ is : -

A saturated solution in $\mathrm{AgA}\left({\mathrm{K}}_{\mathrm{sp}}=3\times {10}^{-14}\right)$ and $\mathrm{Ag}\left({\mathrm{K}}_{\mathrm{sp}}=1\times {10}^{-14}\right)$ has conductivity of $375\times {10}^{-10} {\mathrm{Scm}}^{-1}$ and limiting molar conductivity of ${\mathrm{Ag}}^{+}$ and ${\mathrm{A}}^{-}$ are $60 {\mathrm{Scm}}^2{ \mathrm{mol}}^{-1}$ and $80 {\mathrm{Scm}}^2{ \mathrm{mol}}^{-1}$ respectively then what will be the limiting molar conductivity of $\left({\mathrm{B}}^{-}\mathrm{in} {\mathrm{Scm}}^2{ \mathrm{mol}}^{-1}\right)$

$\mathrm{Na}$-Amalgam is prepared by electrolysis of $\mathrm{aq}.$ $\mathrm{NaCl}$ solution using $10 \mathrm{gm} \mathrm{Hg}$ cathode. How many Faraday's of electricity is required to prepare $18.7\%$ $\mathrm{Na}$-Amalgam. $\left(\mathrm{current} \mathrm{Eff}.=50\%\right)$