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 %