Question

Assume a reaction takes place in a basic solution to form the given products:

[MnO_4^ (aq) + Cl^ (aq) → MnO_2 (s) + Cl_2 (g) ] (unbalanced)
i. Balance the given halfreactions for atoms and charge.
ii. Multiply to balance the charges in the reaction.
iii. Add the equations and simplify to get a balanced equation.
A. Oxidation and Reduction
B. Ionization Energy
C. Isomerization
D. Dehydration

Answer 1

The chemistry question asks for the steps to balance a redox reaction in basic solution between permanganate ions MnO4− and chloride ions Cl−, resulting in MnO2 and Cl2 as products.

Step-by-step explanation:

The question involves balancing redox reactions in basic solutions. The steps to balance the reaction between MnO4− (aq) and Cl− (aq) are as follows:

1. Write the two half-reactions for oxidation and reduction.
2. Balance each half-reaction for elements except for hydrogen and oxygen.
3. Balance for oxygen by adding H2O.
4. Balance for hydrogen by adding hydroxide ions, OH−, since the reaction is in basic solution.
5. Balance for charge by adding electrons.
6. Multiply the half-reactions to equalize the number of electrons transferred in both half-reactions.
7. Combine the half-reactions, cancel out any species that appear on both sides of the equation and simplify.

The balanced chemical equation for the reaction is likely to be:

MnO4− (aq) + 8OH− (aq) + 3Cl− (aq) → MnO2 (s) + 3Cl2 (g) + 4H2O (l)