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2.In the appropriate space after each equation, write the formulas for the oxidant andreductant, and indicate the number of electrons lost per formula from the reductantand the number of electrons gained per formula by the oxidant. When there is noredox occurring, indicate this by writing "no redox"ElectronsElectronsgained perlost perOxidant formula Reductant formulaAg + Cl AgClMg + 2H Mg2H2Ba + 2H20 Ba2 20H + H2CO2 + H20 → H2CO3CO2 C2CO2H202 2H20+ 02137

Question

Number 2 

2.
In the appropriate space after each equation, write the formulas for the oxidant and
reductant, and indicate the number of electrons lost per formula from the reductant
and the number of electrons gained per formula by the oxidant. When there is no
redox occurring, indicate this by writing "no redox"
Electrons
Electrons
gained per
lost per
Oxidant formula Reductant formula
Ag + Cl AgCl
Mg + 2H Mg2
H2
Ba + 2H20 Ba2 20H + H2
CO2 + H20 → H2CO3
CO2 C2CO
2H202 2H20+ 02
137
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2. In the appropriate space after each equation, write the formulas for the oxidant and reductant, and indicate the number of electrons lost per formula from the reductant and the number of electrons gained per formula by the oxidant. When there is no redox occurring, indicate this by writing "no redox" Electrons Electrons gained per lost per Oxidant formula Reductant formula Ag + Cl AgCl Mg + 2H Mg2 H2 Ba + 2H20 Ba2 20H + H2 CO2 + H20 → H2CO3 CO2 C2CO 2H202 2H20+ 02 137

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Step 1

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.

Step 2

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.

Step 3

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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