How many moles of electrons are needed in the balanced equation for the oxidation of ethanol ( $1$ mol) to acetic acid? $(C_{2} H_{5} O H \to C H_{3} C O O H)$

1

No worries! We‘ve got your back. Try BYJU‘S free classes today!

2

No worries! We‘ve got your back. Try BYJU‘S free classes today!

3

No worries! We‘ve got your back. Try BYJU‘S free classes today!

4

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct option is D $4$
The balanced chemical equation for the oxidation reaction is $C_{2} H_{5} O H \to C H_{3} C O O H$ .

The oxidation number of carbon in ethanol is $- 1$ whereas the oxidation number of carbon in acetic acid is $+ 3$ .

Hence, the change in the oxidation number of C is $+ 4$ . Hence, $4$ moles of electrons are needed in the balanced equation for the oxidation of ethanol ( $1$ mol) to acetic acid.

Suggest Corrections

Similar questions

B H_{3}

C_{2} H_{5} O H + C r_{2} O_{7}^{2 -} \to C H_{3} C O O H + C r^{3 +}

C_{2} H_{5} O H

C r_{2} O_{7}^{2 -}

C_{2} H_{5} O H + C r_{2} O_{7}^{2 -} \to C H_{3} C O O H + C r^{3 +}

C_{2} H_{5} O H

C r_{2} O_{7}^{2 -}

H_{2} S O_{4}

(A c_{2} O)

Join BYJU'S Learning Program