Question

Consider the following unbalanced redox equation: (view comment)

Answer 1

\[Mn O_{4^-} (aq) + SbH3 (aq) \rightarrow Mn O_{2}(s) + Sb(s)\]

What is the oxidizing agent in the reaction?

Answer 2

An oxidising agent is substance which oxidises something else.That means that the oxidising agent must be being reduced.Reduction is gain of electrons (OIL RIG).So an oxidising agent must gain electrons.
MnO4-
Oxygen usually has an oxidation number of -2
-2*4=-8
the compound has an overall charge of -1 so Mn must have a charge of +7 -8+7=-1
Hydrogen usually +1except in metal hydrides
SbH3 Sb has a chareg of -3 and H3 is +3 1*3 because three hydrogen atoms are present
MnO2
Mn:+4 O2:-4
The oxidation state of an uncombined element is zero.
Sb(s) has an oxidation number of 0

Answer 3

So the answer is Sb because its oxidation number is 0?

Answer 4

no MnO4 is the oxidising agent

Answer 5

Oh, okay.