Dear student, we answer three parts in a question. I am answering the first three parts. If you need answer for other parts, kindly re-post.
Oxidant is the species in a redox reaction which gets reduced itself and oxidises other species. Thus, the oxidation number of oxidant is reduced and it gains electrons in a redox reaction.
A reductant is a species in a redox reaction which gets oxidised itself and reduces other species. Thus, the oxidation number of the reducatnt is increased and it lose electrons in the redox reaction.
1) In this part,
Oxidant : NO3- because oxidation number of nitrogen has reduced in the given reaction.
Oxidation number of N in NO3- : x + 3 (-2) = -1
x = +5
Oxidation Number of N in NO : x -2 = 0
x = +2
Thus, the change in oxidation number is 3 and the number of electrons gained per formula is 3.
Reductant : Cu
Oxidation number of Cu has increased from 0 to +2
Thus, electrons lost per formula is 2.
2 ) In this part,
Oxidant : Cl2
The oxidation number of Cl is reduced from 0 (in Cl2) to -1 ( in Cl-)
There are two chlorine atoms in the reactant species while one chlorine atom in the product species. Thus, balancing the number of atoms:
Cl2 ( total oxidation number = 0) is changed to 2 Cl- (total oxidation n...
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