Question

Electrolysis of sea-water produces ${Cl}_2\left(g\right)$ at the anode by the oxidation of Cl (aq) ions. What volume of the gas will be produced at STP by current of 1.50 A applied for 90.0 minutes?

• A. 0.313 L
• B. 0.548 L
• C. 0.94 L
• D. 0.470 L

Answer 1

Answer: (C)

0.94 L

Apply farrady law

$W$=$E$*$i$*$t$/$96500$

Where $W$= amount of substance produced

$E$= Molecular weight/ $n$- factor

Put the values

$W$= $71$*$1.5$*$90$*$60$/($2$*$96500$)

$W$= $2.97$ grams

Moles = $2.97$/$71$=$0.042$

$1$mole of $C{l}_2$ containing $22.4$ L volume.

Then,

$0.042$ mole of $C{l}_2$ containing $22.4$*$0.042$ = $0.94$L volume.