$A$ solution of $Fe_{2}(SO_{4})_{3}$ is electrolyzed for '$x$' min with a current of $1.5 \ A$ to deposit $0.3482 \ g$ of $Fe$. The value of $x$ is $.......$. [nearest integer]
Given : $1 \ F = 96500 \ C \ mol^{-1}$
Atomic mass of $Fe = 56 \ g \ mol^{-1}$
Given : $1 \ F = 96500 \ C \ mol^{-1}$
Atomic mass of $Fe = 56 \ g \ mol^{-1}$
- A$10$
- B$20$
- C$25$
- D$35$
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Similar Questions
Match the column :-
Column $I$ (Reduction process) Column $II$ (Charge required) $(a)$ $1$ mol of $MnO_4^-$ to $Mn^{2+}$ $(p)$ $193000$ $C$ $(b)$ $1$ mol of $Cr_2O_7^{2-}$ to $Cr^{3+}$ $(q)$ $289500$ $C$ $(c)$ $1$ mol of $Sn^{4+}$ to $Sn^{2+}$ $(r)$ $482500$ $C$ $(d)$ $1$ mol of $Al^{3+}$ to $Al$ $(s)$ $579000$ $C$
| Column $I$ (Reduction process) | Column $II$ (Charge required) |
|---|---|
| $(a)$ $1$ mol of $MnO_4^-$ to $Mn^{2+}$ | $(p)$ $193000$ $C$ |
| $(b)$ $1$ mol of $Cr_2O_7^{2-}$ to $Cr^{3+}$ | $(q)$ $289500$ $C$ |
| $(c)$ $1$ mol of $Sn^{4+}$ to $Sn^{2+}$ | $(r)$ $482500$ $C$ |
| $(d)$ $1$ mol of $Al^{3+}$ to $Al$ | $(s)$ $579000$ $C$ |
Medium
View Solution$2.644 \ g$ of metal $(M)$ was deposited when $8040 \ C$ of electricity was passed through molten $MF_2$ salt. What is the atomic mass of $M$ $(F = 96500 \ C \ mol^{-1})$ (in $u$)?
When a current of $2 \ A$ is passed through a molten tin salt for $5 \ hours$,$22.2 \ g$ of tin is deposited. What is the oxidation state of tin in the salt? (Atomic weight of $Sn = 118.69$)
Medium
View SolutionWhen a current of $10 \ A$ is passed through molten $AlCl_{3}$ for $1.608 \ minutes$,the mass of $Al$ deposited will be [Atomic mass of $Al = 27 \ g/mol$]:- (in $g$)
An electrolytic cell contains a solution of $Ag_{2}SO_{4}$ and has platinum electrodes. $A$ current is passed until $1.6 \ g$ of $O_{2}$ is liberated at the anode. The amount of silver deposited at the cathode would be ............ $g$.
Medium
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