For the redox reaction : $$MnO_4^ - + {C_2}O_4^{2 - } + {H^ + } \to $$      $$M{n^{2 + }} + C{O_2} + {H_2}O$$     the correct coefficients of the reactants for the balanced reaction are:

	$$MnO_4^ - $$	$${C_2}O_4^{2 - }$$	$${H^ + }$$
(a)	2	5	16
(b)	16	5	2
(c)	5	16	2
(d)	2	16	5

Solution :
TIPS/Formulae :
Balance the reaction by ion electron method.
Oxidation reaction:  $${C_2}O_4^{ - 2} \to 2C{O_2} + 2\left. {{e^ - }} \right] \times 5$$
Reduction reaction :
$$MnO_4^ - + 8{H^ + } + 5{e^ - } \to M{n^{2 + }} + 4{H_2}\left. O \right] \times 2$$
Net reaction :
$$2MnO_4^ - + 16{H^ + } + 5{C_2}O_4^{2 - } \to 2M{n^2} + 10C{O_2} + 8{H_2}O$$