$A$ current $I$ is passed for a time $t$ through a number of voltameters. If $m$ is the mass of a substance deposited on an electrode and $z$ is its electrochemical equivalent,then
- A$\frac{m}{zIt} = 1$
- B$\frac{z}{mIt} = \text{constant}$
- C$\frac{I}{zmt} = \text{constant}$
- D$\frac{It}{zm} = \text{constant}$
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The same quantity of electricity was passed through solutions of salts of elements $X$,$Y$,and $Z$ with atomic masses $7$,$27$,and $48$ respectively. The masses of $X$,$Y$,and $Z$ deposited were $2.1 \ g$,$2.7 \ g$,and $7.2 \ g$ respectively. The valencies of $X$,$Y$,and $Z$ respectively are:
$A$ certain quantity of electricity is passed through an aqueous solution of $AgNO_3$ and a cupric salt solution connected in series. The amount of $Ag$ deposited is $1.08 \ g$. The amount of copper deposited is ............. $g$ (atomic weight of $Cu = 63.5$; $Ag = 108$).
Medium
View SolutionHow much electricity in terms of Faraday is required to produce:
$(i)$ $20.0 \, g$ of $Ca$ from molten $CaCl_2$?
$(ii)$ $40.0 \, g$ of $Al$ from molten $Al_2O_3$?
$(i)$ $20.0 \, g$ of $Ca$ from molten $CaCl_2$?
$(ii)$ $40.0 \, g$ of $Al$ from molten $Al_2O_3$?
Difficult
View SolutionThe atomic weight of $Fe$ is $56$. The weight of $Fe$ deposited from $FeCl_3$ solution by passing $0.6$ Faraday of electricity is $............$ $g$.
Medium
View SolutionThe number of moles of electrons passed when a current of $2 \ A$ is passed through a solution of electrolyte for $20 \ minutes$ is
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