Question

The coefficients when the equation below is balanced are: ____MnO₄^-(aq)+ ____C₂O₄^2-(aq)+ ____H⁺(aq)→ ____Mn²⁺(aq)+ ____CO₂(g)+ ____H₂O(l)

	2, 5, 16, 2, 10, 8
	1, 1, 8, 1, 2, 4
	2, 1, 16, 2, 2, 8
	1, 2, 8, 1, 4, 4

Please provide calculations and explanation. Thank you.

Answer 1

Ans :- 2, 5, 16, 2, 10, 8.

Explanation :-

Follow these four steps :-

Step.1 :- Balance the atoms other than hydrogen (H) and oxygen (O) first for the two half cell reactions i.e. oxidation and reduction separately.

Step.2 :- Balance the oxygen atoms on both sides by adding suitable number of H2O where O contents are less.

Step.3 :- Balance the hydrogen atoms on both the sides by adding suitable number of H+ where H contents are less.

Step.4 :- Balance the charge on both side by adding suitable number of electrons where charge is more.

Reduction half cell reaction is :

MnO4- (aq) + 8H+ (aq) + 5e- ---------------------> Mn2+ (aq) + 4H2O (l) ............(1)

Oxidation half cell reaction is :

C2O42- (aq) --------------------> 2CO2 (g) + 2e- ...........................(2)

Multiply equation (1) by 2 and equation (2) by 5 in order to write overall redox reaction as :

2MnO4- (aq) + 5C2O42- (aq) + 16H+ (aq) -----------------> 2Mn2+ (aq) + 10CO2 (g) + 8H2O (l)