Question

Balance the reaction between Ag and Br₂ to form Br^- and Ag₂O in basic solution. When you have balanced the equation using the smallest integers possible, enter the coefficients of the species shown.

___Ag + ___Br₂ ----> ___Br^- + ___Ag₂O

Water appears in the balanced equation as a ____(reactant, product, neither) with a coefficient of ___. (Enter 0 for neither.)

How many electrons are transferred in this reaction? ____

Answer 1

Oxidation half reaction will be: 2Ag + 2OH^- ---> Ag₂O + 2e^- +  H₂O

Reduction half reaction will be: Br₂ + 2e^----> 2Br^-

Add both the half reactions to get the required balanced equation in basic medium.

2Ag + 2OH^- + Br₂ + 2e^-<----> Ag₂O + 2e^- +  H₂O + 2Br^-

=> 2Ag + Br₂ + 2OH^- <----> 2Br^- + Ag₂O + H₂O

Water appears in the balanced equation as a product with a coefficient of 1.

Two electrons are transferred in this reaction