Copper sulphate solution is electrolysed betw | vedclass

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

Question

(A) The reaction at the anode is: $2H_2O \rightarrow O_2 + 4H^+ + 4e^-$. The equivalent mass of $O_2$ is $E_{O_2} = \frac{32}{4} = 8 \ g/eq$.Number of

Vedclass · Accepted Answer

$6.36$

Vedclass · Answer

(A) The reaction at the anode is: $2H_2O ightarrow O_2 + 4H^+ + 4e^-$. The equivalent mass of $O_2$ is $E_{O_2} = \frac{32}{4} = 8 \ g/eq$.Number of equivalents of $O_2$ liberated = $\frac{1.6 \ g}{8 \ g/eq} = 0.2 \ eq$.According to Faraday's law,the number of equivalents of $Cu$ deposited at the cathode must be equal to the number of equivalents of $O_2$ liberated at the anode.Number of equivalents of $Cu = 0.2 \ eq$.The equivalent mass of $Cu$ is $E_{Cu} = \frac{63.6}{2} = 31.8 \ g/eq$.Mass of $Cu$ deposited = $	ext{Number of equivalents} 	imes E_{Cu} = 0.2 	imes 31.8 = 6.36 \ g$.Therefore,the correct option is $A$.

Copper sulphate solution is electrolysed between two platinum electrodes. $A$ current is passed until $1.6 \ g$ of oxygen is liberated at the anode. The amount of copper deposited at the cathode during the same period is .............. $g$ [At. mass of $Cu = 63.6$]

Similar Questions

What is the charge on tin if $7.375 \ g$ of metallic tin is deposited by the passage of $24125 \ C$ through a solution containing the ion? [Atomic weight of $Sn = 118 \ g/mol$]

How much current in amperes should be passed through a $Na_2SO_4$ solution using graphite electrodes to obtain $250 \ mL$ of $O_2$ gas per minute at $1 \ bar$ pressure and $300 \ K$ temperature (in $A$)? $[R = 0.08314 \ L \ bar \ K^{-1} \ mol^{-1}]$

$A$ current of $2.0 \ A$ is passed for $5 \ hours$ through a molten metal salt,which deposits $22.2 \ g$ of metal (At. wt. $= 177$). The oxidation state of the metal in the metal salt is:

$A$ current of $19296 \ C$ is passed through an aqueous solution of copper sulphate using copper electrodes. What is the mass (in $g$) of copper deposited at the cathode? (Molar mass of $Cu = 63.5 \ g \ mol^{-1}$)

How much charge in Coulombs is required for the oxidation of $1 \ mol$ of $H_2O$ to $O_2$?

Vedclass Test Series

Exam Paper Generator

Online Exam Module