Question

Balancing Redox Equations: Half-reaction Method

Potassium permanganate, KMnO4, is a powerful oxidizing agent. The products of a given redox reaction with the permanganate ion depend on the reaction conditions used.In basic solution, the following equation represents the reaction of this ion with a solution containing sodium fluoride:
MnO4^-(aq)+F^-(aq)–>MnO2(s)+F2(aq)

Since this reaction takes place in basic solution, and will be shown in the reaction. Places for these species are indicated by the blanks in the following restatementof the equation:
MnO4^-(aq)+F^-(aq)+____–>MnO2(s)+F2(aq)+____
What are the coefficients of the reactants and products in the balanced equation above? Remember to include and in the blanks where appropriate.

**In the hints, it gives this equation at the end:
2Mn04^-(aq)+6F^-(aq)+8H^+(aq)+8OH^-(aq)—>2MnO2(s)+3F2(aq)+4H2O(l)+8OH^-(aq)

Finally, cancel any water molecules appearing both as reactants and products to complete the mass balance.

Solutions

Expert Solution
No answers


Submit Your Answer