The number of coulombs required for the depos | vedclass

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

Question

(A) The reaction for the deposition of silver is: $Ag^+ + e^- \rightarrow Ag(s)$.From the stoichiometry,$1 \ mole$ of electrons is required to deposit

Vedclass · Accepted Answer

$96500$

Vedclass · Answer

(A) The reaction for the deposition of silver is: $Ag^+ + e^- \rightarrow Ag(s)$.From the stoichiometry,$1 \ mole$ of electrons is required to deposit $1 \ mole$ of silver.The molar mass of silver $(Ag)$ is $107.870 \ g/mol$.Thus,$107.870 \ g$ of silver corresponds to $1 \ mole$ of silver.Since $1 \ mole$ of electrons carries a charge of $1 \ Faraday$,which is equal to $96500 \ C$,the charge required is $96500 \ C$.

The number of coulombs required for the deposition of $107.870 \ g$ of silver is

Similar Questions

What is the quantity of electricity required to produce $4.8 \ g$ of $Mg$ (molar mass $= 24 \ g \ mol^{-1}$) from its salt solution (in $F$)?

In the electrolysis of water,one Faraday of electrical energy would evolve

The mass of zinc produced by the electrolysis of zinc sulphate solution with a steady current of $0.015 \ A$ for $15$ minutes is . . . . . . $ \times 10^{-4} \ g$. (Atomic mass of zinc $= 65.4 \ amu$)

The Faraday constant is $......$

How much time is required for complete decomposition of $4 \, \text{moles}$ of water using $4 \, \text{A}$ current?

Vedclass Test Series

Exam Paper Generator

Online Exam Module