How long will it take for a uniform current of $6.0$ ampere to deposit $78.0$ gold from a solution of $A u C l_{4}^{-}$ ? What mass of chlorine gas will be formed simultaneously at the anode in the electroytic cell?

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Solution

$i = 6.0 A$
$w = 78.02 A u$
$A u C l_{4}^{-} \to A u + 2 C l_{2} + e^{-}$
$n_{f} = 2$
$w_{A u} = Z i t$
$78.0 = \frac{196.96}{3 \times F} \times 6 \times t$
$t = 19107.94 s e c$
$= 318.4 m i n$
$f o r C l_{2}$
$= \frac{70.9}{1 \times 96500} \times 6 \times 19107.94$
$w t . o f C l_{2} = 84.23334 g$

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Similar questions

Q. How long will it take for a uniform current of 6.0 ampere to deposit 78.0 g gold from a solution of

A u C l_{4}^{-}

A uniform current of 6.0A is required to deposit 78 g of gold from a solution of $A u C l_{4}^{-}$ . What mass of chlorine gas will be formed simultaneously at the anode of the electrolytic cell?

Q. How much time will it take for a uniform current of

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How long will it take for a uniform current of 6.0 ampere to deposit 78.0 gold from a solution of AuCl−4? What mass of chlorine gas will be formed simultaneously at the anode in the electroytic cell?

i=6.0Aw=78.02AuAuCl−4→Au+2Cl2+e− nf=2wAu=Zit78.0=196.963×F×6×tt=19107.94sec=318.4minforCl2=70.91×96500×6×19107.94wt.ofCl2=84.23334g

How long will it take for a uniform current of $6.0$ ampere to deposit $78.0$ gold from a solution of $A u C l_{4}^{-}$ ? What mass of chlorine gas will be formed simultaneously at the anode in the electroytic cell?

$i = 6.0 A$
$w = 78.02 A u$
$A u C l_{4}^{-} \to A u + 2 C l_{2} + e^{-}$
$n_{f} = 2$
$w_{A u} = Z i t$
$78.0 = \frac{196.96}{3 \times F} \times 6 \times t$
$t = 19107.94 s e c$
$= 318.4 m i n$
$f o r C l_{2}$
$= \frac{70.9}{1 \times 96500} \times 6 \times 19107.94$
$w t . o f C l_{2} = 84.23334 g$