One Faraday of electricity liberates x times | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) The electrode reaction for the reduction of copper ions is: $Cu^{2+} + 2e^{-} \rightarrow Cu$.According to the stoichiometry of the reaction,$2 \

Vedclass · Accepted Answer

$5$

Vedclass · Answer

(B) The electrode reaction for the reduction of copper ions is: $Cu^{2+} + 2e^{-} ightarrow Cu$.According to the stoichiometry of the reaction,$2 \ Faraday$ of electricity is required to deposit $1 \ mol$ (or $1 \ 	ext{gram atom}$) of copper.Therefore,$1 \ Faraday$ of electricity will deposit $1/2 = 0.5 \ 	ext{mol}$ of copper.Since $0.5 \ 	ext{mol} = 0.5 \ 	ext{gram atom}$,we can express this as $5 	imes 10^{-1} \ 	ext{gram atom}$.Comparing this with $x 	imes 10^{-1}$,we get $x = 5$.

One Faraday of electricity liberates $x \times 10^{-1}$ gram atom of copper from copper sulphate,$x$ is . . . . . . .

Similar Questions

The electrochemical equivalent of magnesium is $0.126 \ mg/C$. $A$ current of $5 \ A$ is passed in a suitable solution for $1 \ hour$. The mass of magnesium deposited will be ........... $gm$.

The amount of copper metal deposited at cathode on passing electric current of $500 \ mA$ for $20 \ min$ in cupric chloride solution is ............ $g$

When a current of $9.65 \ A$ is passed for $10 \ \text{minutes}$,$3.0 \ g$ of metal is deposited. What is the equivalent weight of the metal?

Find the number of faradays of electricity required to produce $45 \ g$ of $Al$ from molten $Al_2O_3$. (in $F$)

When $9.65 \ C$ of electricity is passed through a solution of silver nitrate (atomic weight of $Ag = 108$),the amount of silver deposited is $............ \ mg$.

Vedclass Test Series

Exam Paper Generator

Online Exam Module