For the redox reaction, #MnO_4^(-) + C_2O_4^(2-) + H^(+) -> Mn^(2+) + CO_2 +H_2O# The correct coefficients of the reactants for the balanced reaction are respectively, #MnO_4^-# , #C_2O_4^(2-)# , #H^+# ? :-
(1) 2,5,16
(2) 16,3,12
(3) 15,16,12
(4) 2,16,5
(1) 2,5,16
(2) 16,3,12
(3) 15,16,12
(4) 2,16,5
3 Answers
This is a lot of work for a multiple choice question.... I make it
Explanation:
Permanganate,
Oxalate anion,
And we take
..to give finally....
An examiner is being lazy if they set a question like this....
(1)
Explanation:
at first you must find the elements that change their oxidation number end calculate these numbers before and after the reaction:
Mn goes from +7 to +2 and it gain 5 electrons:
look that you must balance the atoms of oxygen with water and the atoms of Hydrogen with ion
while C goes from + 3 to +4 and it lost 1 electron for each atoms
but you must balance the number of electrons in the two reactions, so you mustmoltiplicate for 2 the first and for 5 the second reaction:
now you summ the two reactions and you have:
semplifying the electrons, you get
that is what you were looking for
(1) 2,5,16
Explanation:
Because of the
Looking at the equation, there must be a significantly smaller number of
One can definitely try to balance the equation, but in this case it is unnecessary.