Which of the following reactions will be spon | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) For a reaction to be spontaneous in an electrochemical cell,the cell potential $E_{cell}^0$ must be positive.$E_{cell}^0 = E_{cathode}^0 - E_{anod

Vedclass · Accepted Answer

$2Br^- + Cl_2 \rightarrow Br_2 + 2Cl^-$

Vedclass · Answer

(B) For a reaction to be spontaneous in an electrochemical cell,the cell potential $E_{cell}^0$ must be positive.$E_{cell}^0 = E_{cathode}^0 - E_{anode}^0$.Given $E_{Cl_2 \mid 2Cl^-}^0 = 1.36 \ V$ and $E_{Br_2 \mid 2Br^-}^0 = 1.09 \ V$.For option $B$: $2Br^- + Cl_2 \rightarrow Br_2 + 2Cl^-$.Here,$Cl_2$ is reduced to $Cl^-$ (cathode) and $Br^-$ is oxidized to $Br_2$ (anode).$E_{cell}^0 = E_{Cl_2 \mid 2Cl^-}^0 - E_{Br_2 \mid 2Br^-}^0 = 1.36 \ V - 1.09 \ V = 0.27 \ V$.Since $E_{cell}^0 > 0$,the reaction is spontaneous.

Which of the following reactions will be spontaneous in an electrochemical cell constructed from the given standard electrode potentials: $E_{Cl_2 \mid 2Cl^-}^0 = 1.36 \ V$ and $E_{Br_2 \mid 2Br^-}^0 = 1.09 \ V$?

Similar Questions

For the following cell reaction,$Ag | Ag^{+} | AgCl | Cl^{-} | Cl_2, Pt$
$\Delta G_f^{\circ}(AgCl) = -109 \ kJ/mol$
$\Delta G_f^{\circ}(Cl^{-}) = -129 \ kJ/mol$
$\Delta G_f^{\circ}(Ag^{+}) = 78 \ kJ/mol$
$E^{\circ}$ of the cell is

Given $E^{0}_{Fe^{2+} | Fe} = -0.44 \, V$ and $E^{0}_{Sn^{2+} | Sn} = -0.14 \, V$,calculate $E^{0}_{cell}$ for the reaction $Fe^{2+} + Sn \rightarrow Fe + Sn^{2+}$.

Which among the following reactions will take place spontaneously?

The standard electrode potential is measured by

Discuss the method to determine the cell potential of any cell when a standard hydrogen electrode is considered as the anode,with a suitable example.

Vedclass Test Series

Exam Paper Generator

Online Exam Module