Consider the following redox reaction taking place in acidic medium BH_ 4 ^ - (a q)+ClO_ 3 ^ - (a q) H_ 2 BO_ 3 ^ - (a q)+Cl^ - (a q) If the Nernst equation for the above balanced reaction is E_ cell =E_ cell ^ - RT nF

Correct answer: 0 3BH_4^- + 4ClO_3^- 4Cl^- + 3H_2BO_3^- + 3H_2O n-factor = 8 moles = 3 n = 3 × 8 = 24

JEE Main 202628 JanuaryMorning Shift

JEE Main 2026 · 28 January · Morning Shift · Chemistry · Electrochemistry

Consider the following redox reaction taking place in acidic medium...

Consider the following redox reaction taking place in acidic medium

\mathrm{BH}_{4}^{-}(a q)+\mathrm{ClO}_{3}^{-}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{BO}_{3}^{-}(a q)+\mathrm{Cl}^{-}(a q)

If the Nernst equation for the above balanced reaction is

\mathrm{E}_{\text{cell }}=\mathrm{E}_{\text{cell }^{\circ}-\frac{\mathrm{RT}}{\mathrm{nF}} \ln \mathrm{Q} , then the value of

is

\_\_\_\_

. (Nearest integer)

3BH_4^- + 4ClO_3^- \longrightarrow 4Cl^- + 3H_2BO_3^- + 3H_2O

n-factor

= 8

moles

= 3

\therefore n = 3 \times 8 = 24