Embibe Experts Solutions for Chapter: Electrochemistry, Exercise 1: Maharashtra Board-2018

Represent a cell consisting of ${\mathrm{Mg}}^{2+}$ | $\mathrm{Mg}$ half cell and ${\mathrm{Ag}}^{+}$ | $\mathrm{Ag}$ half cell and write the cell reaction.

$(\mathrm{E}{°}_{\mathrm{Ag}}=0.799 \mathrm{V}, \mathrm{E}{°}_{\mathrm{Mg}}=-2.37 \mathrm{V})$

How much quantity of electricity in coulomb is required to deposit $1.346 \times {10}^{-3} \mathrm{kg} \mathrm{of} \mathrm{Ag}$ in $3.5$ minutes from ${\mathrm{AgNO}}_3$ solution? (Given : Molar mass of Ag is $108\times {10}^{-3} \mathrm{kg} {\mathrm{mol}}^{-1}$ )

The S.I. unit of cell constant for conductivity cell is :

How many faradays of electricity are required to produce $6 \mathrm{g}$ of $\mathrm{Mg}$ from ${\mathrm{MgCl}}_2$?

The molar conductivity of $0.05 \mathrm{M} {\mathrm{BaCl}}_2$ solution at $25°\mathrm{C}$ is $223 {\mathrm{\Omega }}^{-1 }{\mathrm{cm}}^2{\mathrm{mol}}^{-1}$. What is its conductivity?

Define electrochemical series. Write its applications.

Define the term:

Electrochemical series

Define the term: Corrosion
Write two applications of electrochernical series.