In an electroplating experiment,$m \ g$ of silver is deposited when $4 \ A$ of current flows for $2 \ min$. The amount (in $g$) of silver deposited by $6 \ A$ of current flowing for $40 \ s$ will be:
- A$4 \ m$
- B$m/2$
- C$m/4$
- D$2 \ m$
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Similar Questions
The quantity of charge required to obtain $2$ moles of aluminium from $Al_2O_3$ is: (in $F$)
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 SolutionHow long would it take to reduce completely $80 \ mL$ of $0.1 \ M$ $Fe_2(SO_4)_3$ to $FeSO_4$ by passing a current of $2 \ A$?
Medium
View SolutionIn the process of electroplating,$m \ g$ of silver is deposited when $4 \ A$ of current flows for $2 \ min$. The amount (in $g$) of silver deposited by $6 \ A$ of current flowing for $40 \ s$ will be
Medium
View SolutionIn a copper voltameter experiment,current is decreased to one-fourth of the initial value but it is passed for four times the earlier duration. The amount of copper deposited will be:
Difficult
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