What is achieved by Faraday using the principles of electrolysis?
- A$A$. Separation of metals from ores
- B$B$. Electroplating
- C$C$. Extraction of non-metals
- D$D$. All of the above
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Similar Questions
When $10 \,A$ current is passed for $80 \,min$, the volume of hydrogen gas liberated at $STP$ is: (in $\,L$)
$6.5 \, g$ of $Mg$ is deposited during the electrolysis of fused $MgCl_2$. What will be the volume of chlorine gas (in $L$) discharged at the electrode at $STP$?
Easy
View SolutionMatch the column :-Column $I$ (Reduction process) Column $II$ (Charge required) $(a)$ $1$ mol of $MnO_4^-$ to $Mn^{2+}$ $(p)$ $193000$ $C$ $(b)$ $1$ mole of $Cr_2O_7^{2-}$ to $Cr^{3+}$ $(q)$ $289500$ $C$ $(c)$ $1$ mole of $Sn^{4+}$ to $Sn^{2+}$ $(r)$ $482500$ $C$ $(d)$ $1$ mole of $Al^{3+}$ to $Al$ $(s)$ $579000$ $C$
| Column $I$ (Reduction process) | Column $II$ (Charge required) |
|---|---|
| $(a)$ $1$ mol of $MnO_4^-$ to $Mn^{2+}$ | $(p)$ $193000$ $C$ |
| $(b)$ $1$ mole of $Cr_2O_7^{2-}$ to $Cr^{3+}$ | $(q)$ $289500$ $C$ |
| $(c)$ $1$ mole of $Sn^{4+}$ to $Sn^{2+}$ | $(r)$ $482500$ $C$ |
| $(d)$ $1$ mole of $Al^{3+}$ to $Al$ | $(s)$ $579000$ $C$ |
Difficult
View SolutionWhich is the weight of $Al$ deposited at cathode when $1 \ A$ current is passed through molten $AlCl_3$ for $9650 \ s$ (in $g$)?
(Atomic mass of $Al = 27$)
(Atomic mass of $Al = 27$)
According to the first law of Faraday,the weight of a substance discharged at the electrode is:
Easy
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