In a certain electrolysis experiment,0.650 g | vedclass

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

Question

(A) According to Faraday's second law of electrolysis,when cells are connected in series,the mass of substances deposited is proportional to their equ

Vedclass · Accepted Answer

$0.635$

Vedclass · Answer

(A) According to Faraday's second law of electrolysis,when cells are connected in series,the mass of substances deposited is proportional to their equivalent masses: $\frac{W_{Zn}}{E_{Zn}} = \frac{W_{Cu}}{E_{Cu}}$Equivalent mass of $Zn = \frac{	ext{Molar mass}}{	ext{Valency factor}} = \frac{65}{2} = 32.5 \ g \ eq^{-1}$Equivalent mass of $Cu = \frac{	ext{Molar mass}}{	ext{Valency factor}} = \frac{63.5}{2} = 31.75 \ g \ eq^{-1}$Substituting the values: $\frac{0.650}{32.5} = \frac{W_{Cu}}{31.75}$$W_{Cu} = \frac{0.650 	imes 31.75}{32.5} = 0.635 \ g$

In a certain electrolysis experiment,$0.650 \ g$ of zinc is deposited in a cell having $ZnSO_4$ solution. Calculate the mass of $Cu$ deposited in another cell having $CuSO_4$ solution arranged in series with the first cell (in $g$)? (Molar mass of $Zn = 65 \ g \ mol^{-1}$,$Cu = 63.5 \ g \ mol^{-1}$)

Similar Questions

$A$ solution of copper sulphate $(CuSO_4)$ is electrolysed for $10 \, \text{minutes}$ with a current of $1.5 \, \text{amperes}$. The mass of copper deposited at the cathode (atomic mass of $Cu = 63 \, u$) is ............ $g$.

What is the number of faraday required to form $1 \ mol \ H_2$ by reduction of $H^{+}$ ions?

How much volume of oxygen at $STP$ will be liberated by $2$ $ampere$ flowing for $3$ $minutes$ and $13$ $seconds$ through acidified water? (in $cc$)

To deposit $0.6354 \ g$ of copper by electrolysis of aqueous cupric sulphate solution,the amount of electricity required (in coulombs) is

In the electrolysis of $CuCl_2$,a current of $2.0 \ A$ is passed through the solution at $1 \ bar$ pressure and $300 \ K$ temperature for $1 \ hour$. Calculate the amount of product obtained at the anode and cathode. $[Cu = 63.5, \ Cl = 35.5, \ R = 0.08314 \ L \ bar \ K^{-1} \ mol^{-1}]$

Vedclass Test Series

Exam Paper Generator

Online Exam Module