Question

Anthracene can be electrolytically oxidised to anthraquinone.
What mass of anthraquinone can be produced by the passage of $1$ ampere current for an hour at $100$% efficiency?

• A. $3.654g$.
• B. $2g$.
• C. $12g$.
• D. $1.2932g$.

Answer 1

The correct option is D $1.2932g$.

Here,

$w=$$\frac{EIt}{96500}$

When anthracene is converted into anthraquinone then 6 moles of electron are required to completely oxidize 1 mole of anthracene.

$w=$$\frac{208\times 1\times 60\times 60}{6\times 96500}$

$w=1.2932g$