Energy of activation is lower for reaction :

R C H_{2} ⨁ O H_{2} \to R ⨁ C H_{2}

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

R_{2} C H ⨁ O H_{2} \to R_{2} ⨁ C H

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

R_{3} C ⨁ O H_{2} \to R_{3} ⨁ C

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

all have same

E_{a c t}

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

Open in App

Solution

The correct option is B $R_{3} C ⨁ O H_{2} \to R_{3} ⨁ C$
Formation of a more stable carbocation result in lower activation energy and faster ionization. The stability of carbocations increases as we go from primary to secondary to tertiary carbons, due to carbons (alkyl groups in particular) as being “electron-releasing” groups through inductive effects. Therefore option C is the correct answer.

Suggest Corrections

Similar questions

\to

H_{3} C - + O H_{2} \to C H_{3}^{+} + H_{2} O

(C H_{3})_{3} C - + O H_{2} \to (C H_{3})_{3} C^{+} + H_{2} O

(C H_{3})_{2} C - + O H_{2} \to (C H_{3})_{2} C H^{+} + H_{2} O

C_{2} H_{5} {O H}_{2} H_{5} + C O \begin{matrix} {B F}_{3500 a t m s} ⟶ 150^{\circ} C \end{matrix} X

X

Why Ca(OH2) + CO2 👉 CaCO3 + H2O?

Why is water H₂O and not OH₂ & NaCl and not ClNa?

Join BYJU'S Learning Program