K L Chugh Solutions for Chapter: Electrochemistry, Exercise 14: Follow Up Problems

For how long a current of $1.5$ amperes, has to be passed through the electrolyte in order to deposit $1.5 \mathrm{g}$ of $\mathrm{Al}$ , when the electrode reaction is

${\mathrm{Al}}^{3+}+3{\mathrm{e}}^{-}⟶\mathrm{Al}$   (Atomic mass of $\mathrm{Al}=27$)

When a current of $0.75 \mathrm{A}$ is passed through a ${\mathrm{CuSO}}_4$ solution for $25$ minutes, $0.369 \mathrm{g}$ of copper is deposited at the cathode. Calculate the atomic mass of copper.

Write anode and cathode reactions for the electrolysis of water. How much charge will be transported for the decomposition of $3.6 \mathrm{g}$ of ${\mathrm{H}}_2\mathrm{O}?\left(\mathrm{F}=96500 \mathrm{C} {\mathrm{mol}}^{-1}\right)$

How much charge is required for the following reduction of:

$1 \mathrm{mol}$ of ${\mathrm{Al}}^{3+}$ to $\mathrm{Al}$

How much charge is required for the following reduction of:$1 \mathrm{mol}$ of ${\mathrm{Cu}}^{2+}$ to $\mathrm{Cu}$?

A current of $1.5$ amperes is passed for $10$ minutes through a solution of ${\mathrm{CuSO}}_4.$ What is the mass of copper deposited at the cathode ? (Atomic mass of $\mathrm{Cu}=63.5$)