Answer :
(a) The limiting reactant is, 
(b) The mass of excess reactant is, 1.7646 g
(c) The theoretical yield of NO is, 2.616 g
(d) The percent yield of the reaction is, 37.46 %
Explanation : Given,
Mass of
= 3.25 g
Mass of
= 3.50 g
Molar mass of
= 17 g/mole
Molar mass of
= 32 g/mole
Molar mass of
= 30 g/mole
First we have to calculate the moles of
and
.


Now we have to calculate the limiting and excess reagent.
The balanced chemical reaction is,

From the balanced reaction we conclude that
As, 5 moles of
react with 4 mole of 
So, 0.109 moles of
react with
moles of 
From this we conclude that,
is an excess reagent because the given moles are greater than the required moles and
is a limiting reagent and it limits the formation of product.
The limiting reactant is, 
Excess moles of
= 0.191 - 0.0872 = 0.1038 mole
Now we have to calculate the mass of
.


The mass of excess reactant = 1.7646 g
Now we have to calculate the moles of
.
As, 5 moles of
react with 4 mole of 
So, 0.109 moles of
react with
moles of 
Now we have to calculate the mass of
.


Now we have to calculate the percent yield of 

The percent yield of the reaction is, 37.46 %