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When the following equation is balanced properly under acidic conditions, what are the coefficients of the species shown?Mn2+HNO3+NO+(reactant, product, neither) with a coefficient ofEnter 0 for neither.)Water appears in the balanced equation as aHow many electrons are transferred in this reaction?

Question
When the following equation is balanced properly under acidic conditions, what are the coefficients of the species shown?
Mn2+
HNO3+
NO+
(reactant, product, neither) with a coefficient ofEnter 0 for neither.)
Water appears in the balanced equation as a
How many electrons are transferred in this reaction?
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When the following equation is balanced properly under acidic conditions, what are the coefficients of the species shown? Mn2+ HNO3+ NO+ (reactant, product, neither) with a coefficient ofEnter 0 for neither.) Water appears in the balanced equation as a How many electrons are transferred in this reaction?

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Step 1

For balancing a redox reaction, certain steps are followed.

STEP 1 : Writing the skeletal equation and calculating the oxidation number on all atoms.

For calculating oxidation number, certain rules need to be followed:

Oxidation no. of O in almost all of its compounds is -2.

Oxidation no. of H in most of its compounds is +1.

The sum of oxidation numbers of all atoms in a species is equal to the total charge on the species.

NO:

Let oxidation no. of N be x:      x-2 = 0     or x = +2

MNO4-:

Let oxidation no. of Mn be y           y + 4(-2)=-1    or         y = +7

HNO3       : Let oxidation number of N be z

1+z+3(-2)=0     or z = +5

 

Step 2

STEP 2 : Separating the equation into two half reactions-oxidation (increase in oxidation no.)  half reaction and reduction (decrease in oxidation no.) half reaction.

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Step 3

STEP 3: Balancing atoms other than O and H in the two half reactions:

I...

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