Embibe Experts Solutions for Chapter: Electrochemistry, Exercise 4: Exercise 4

The cell constant of a given cell is $0.47 {\mathrm{cm}}^{-1}.$ The resistance of a solution placed in this cell is measured to be $31.6 \mathrm{ohm}.$ The conductivity of the solution (in $\mathrm{S} {\mathrm{cm}}^{-1}$ where, $\mathrm{S}$ has usual meaning) is

$4.5 \mathrm{g}$ of aluminium (atomic mass $27 \mathrm{amu})$ is deposited at cathode from ${\mathrm{Al}}^{3+}$ solution by a certain quantity of electric charge. The volume of hydrogen produced at $\mathrm{STP}$ from ${\mathrm{H}}^{+}$ ions in solution by the same quantity of electric charge will be.

The number of electrons delivered at the cathode during electrolysis by a current of $1 \mathrm{ampere}$ in $60 \mathrm{seconds}$ is: (charge on electron$=$${\mathrm{1.60\times 10}}^{\mathrm{-19}} \mathrm{C}$ )

The standard reduction potential for ${\mathrm{Zn}}^{\mathrm{2+}}/\mathrm{Zn}, {\mathrm{Ni}}^{\mathrm{2+}}/\mathrm{Ni} \text{and} {\mathrm{Fe}}^{\mathrm{2+}}/\mathrm{Fe}$ are $-0.76 \mathrm{V}, -0.23 \mathrm{V} \mathrm{and} -0.44 \mathrm{V}$, respectively. The reaction $\mathrm{X}+{\mathrm{Y}}^{+2}\stackrel{}{\to } {\mathrm{X}}^{2+}+\mathrm{Y}$ will be spontaneous when ______.

Resistance of $0.2 \mathrm{M}$ solution of an electrolyte is $50 \mathrm{\Omega }$. The specific conductance of the solution is $1.4 \mathrm{S} {\mathrm{m}}^{-1}$. The resistance of $0.5 \mathrm{M}$ solution of the same electrolyte is $280 \mathrm{\Omega }$. The molar conductivity of $0.5 \mathrm{M}$ solution of the electrolyte in $\mathrm{S} {\mathrm{m}}^2 {\mathrm{mol}}^{-1}$ is

The equivalent conductance of $\mathrm{NaCl}$ at concentration $\mathrm{C}$ and at infinite dilution are ${\mathrm{\lambda }}_{\mathrm{C}}$ and ${\mathrm{\lambda }}_{\infty }$ respectively. The correct relationship between ${\mathrm{\lambda }}_{\mathrm{C}}$ and ${\mathrm{\lambda }}_{\infty }$ is given as

The metal that cannot be obtained by electrolysis of an aqueous solution of its salts is?

How long (approximate) should water be electrolysed by passing through $100$ amperes current so that the oxygen released can completely burn $27.66 \mathrm{g}$ of diborane? (Atomic weight of $\mathrm{B}=10.8 \mathrm{u}$)