Write oxidation and reduction half - reaction equations and add them to produce

Question

Write oxidation and reduction half - reaction equations and add them to produce the net ionic equation for the reaction between permanganate and chloride ions in acidic medium. The "skeletons" are MnO_4^- rightarrow Mn^2+ and CI^- rightarrow Cl_2. Write oxidation and reduction half - reaction equations and add them to produce the net ionic equation for the halogen - halide reaction involving chlorine and iodide that did occur. Write the four reduction half - reactions for Part 2 in which the oxidizing agents are arranged in order of decreasing strength from top to bottom (i.e. Cl_2 + 2e^- 2CI^-). Be sure to include the permanganate ion also.

Explanation / Answer

Oxidation Half reaction:

(i) Cl- ---------------> Cl2

(ii) Balance atoms other than O and H

2 Cl- ------------> Cl2

(iii) To balance charge add electrons at mor positive side

2 Cl- -----------> Cl2 + 2 e

Reduction Half reaction:

(i) MnO4- -------------> Mn2+

(ii) To balance Oxygens in acidic medium add water molecules at required side.

MnO4- ----------------> Mn2+ + 4 H2O

(iii) To balance hydrogens in acidic medium add H+ ions at required side.

MnO4- + 8 H+ --------------> Mn2+ + 4 H2O

(iv) To balnce charge add electrons at more positive charge side.

MnO4- + 8 H+ + 5 e --------------> Mn2+ + 4 H2O

To get the final net ionic equation, do oxidation half *5 + reduction half * 2

10 Cl- -------------> 5 Cl2 + 10 e

2 MnO4- + 16 H+ + 10 e ----------> 2 Mn2+ + 8 H2O

Net ionic equation: 2 MnO4- + 10 Cl- + 16 H+ --------------> 2 Mn2+ + 5 Cl2 + 8 H2O

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