What current strength in amp will be required | vedclass

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

Question

(C) The reaction for the liberation of chlorine is: $2Cl^- \rightarrow Cl_2 + 2e^-$. The molar mass of $Cl_2$ is $71 \ g/mol$. The mass of $Cl_2$ libe

Vedclass · Accepted Answer

$7.55$

Vedclass · Answer

(C) The reaction for the liberation of chlorine is: $2Cl^- ightarrow Cl_2 + 2e^-$. The molar mass of $Cl_2$ is $71 \ g/mol$. The mass of $Cl_2$ liberated is $10 \ g$. The number of moles of $Cl_2$ is $n = \frac{10}{71} \approx 0.1408 \ mol$. According to the reaction,$2 \ mol$ of electrons are required to produce $1 \ mol$ of $Cl_2$. Total charge $Q = n 	imes 2 	imes F = 0.1408 	imes 2 	imes 96500 \ C \approx 27174.6 \ C$. Time $t = 1 \ hour = 3600 \ s$. Current $I = \frac{Q}{t} = \frac{27174.6}{3600} \approx 7.548 \ A \approx 7.55 \ A$.

What current strength in $amp$ will be required to liberate $10 \ g$ of chlorine from $NaCl$ solution in one hour?

Similar Questions

On passing $3 \ A$ of electricity for $50 \ minutes$,$1.8 \ g$ of metal deposits. The equivalent mass of the metal is:

In electrolysis,if the duration of the passage of current is doubled,the mass liberated is

On passing $96500 \ C$ of charge through a $CuSO_4$ solution,the amount of copper liberated is:

When the same quantity of electricity is passed through aqueous solutions of $AgNO_3$ and $CuSO_4$,if the number of atoms of $Ag$ and $Cu$ deposited are $x$ and $y$ respectively,then determine the correct relationship.

The number of Faradays $F$ required to produce $20 \ g$ of calcium from molten $CaCl_2$ (Atomic mass of $Ca = 40 \ g \ mol^{-1}$) is

Vedclass Test Series

Exam Paper Generator

Online Exam Module