Question

Balance each redox reaction in basic solution using the half reaction method. (Please provide step by step solution because I'm lost in this area)

O₂ + Cr³⁺ → H₂O₂ + Cr₂O₇^2-

Te + NO₃^- → TeO₃^2- + N₂O₄

IO₃^-+Re→ReO₄^- +IO^-

Pb²⁺+IO^3-→ PbO₂ +I₂

Cr₂O₇^2- + Hg → Hg²⁺ + Cr³⁺

Answer 1

• split the whole equation into oxidation half and reduction half equation basing on their oxidation states.
• Balance each atom on bothe side except oxygen and hydrogen
• The side deficient in hydrogen should be added with required number of water and the opposite side should be added with same number of OH^- ion.
• The side excess in oxygen should be added with required number of oxygen and the opposite side should be added with double the number of OH^- ion
• Balance the charges on both side of each half reaction by either adding or subtracting required number of electrons