Answer :
(a) Limiting reactant =
(b) The excess reactant =
(c) The percent of excess reactant is, 50.87 %
(d) The percent yield of or percent conversion of
to
is, 38.80 %
(e) The mass of produced is, 1066.42 lb
Explanation : Given,
Mass of = 200 lb = 90718.5 g
conversion used : (1 lb = 453.592 g)
Mass of = 1000 lb = 453592 g
Molar mass of = 7.95 g/mole
Molar mass of = 117.17 g/mole
Molar mass of = 27.66 g/mole
Molar mass of = 42.39 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, 6 moles of react with 1 mole of
So, 11411.13 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.
Moles of remaining excess reactant = 3871.23 - 1901.855 = 1969.375 moles
Total excess reactant = 3871.23 moles
Now we have to determine the percent of excess reactant .
The percent of excess reactant is, 50.87 %
Now we have to calculate the moles of .
As, 6 moles of react to give 1 mole of
So, 11411.13 moles of react to give
moles of
Now we have to calculate the mass of .
Now we have to calculate the percent yield of .
The percent yield of or percent conversion of
to
is, 38.80 %
Now we have to calculate the moles of .
As, 6 moles of react to give 6 mole of
So, 11411.13 moles of react to give 11411.13 moles of
Now we have to calculate the mass of .
The mass of produced is, 1066.42 lb