Which of the following is the correctly balanced redox reaction for H2O2(aq) + ClO2(aq) → ClO₂⁻(aq) + O₂(g) in a basic solution?

Complete and balance the following equations, and identify the oxidizing and reducing agents:

a. MnO4−(𝑎𝑞)+CH3OH(𝑎𝑞)⟶Mn2+(𝑎𝑞)+HCOOH(𝑎𝑞)(acidic solution)

b. As2O3(𝑠)+NO3−(𝑎𝑞)⟶H3AsO4(𝑎𝑞)+N2O3(𝑎𝑞)(acidic solution)

c. Pb(OH)42−(𝑎𝑞)+ClO−(𝑎𝑞)⟶PbO2(𝑠)+Cl−(𝑎𝑞)(basic solution)

Complete and balance the following equations, and identify the oxidizing and reducing agents. (Recall that the O atoms in hydrogen peroxide, H2O2, have an atypical oxidation state.)

a. S(s) + HNO3(aq) → H2SO3(aq) + N2O(g) (acidic solution)

b. BrO3-(aq) + N2H4(g) → Br-(aq) + N2(g) (acidic solution)

c. H2O2(aq) + ClO2(aq) → ClO20(aq) _ O2(g) (basic solution)

Complete and balance the following half-reactions in basic solution. In each case, indicate whether the half-reaction is an oxidation or a reduction. c. Cr(OH)3(𝑠)⟶CrO42−(𝑎𝑞)

Balance each redox reaction occurring in basic aqueous solution. c. Cl₂(g) → Cl^–(aq) + ClO^–(aq)