Answer : The percent yield of the reaction is, 76.34 %
Explanation : Given,
Pressure of  and
 and  = 25.0 atm
 = 25.0 atm
Temperature of  and
 and  =
 = 
Volume of  = 1050 L per min
 = 1050 L per min
Volume of  = 1550 L per min
 = 1550 L per min
R = gas constant = 0.0821 L.atm/mole.K
Molar mass of  = 30 g/mole
 = 30 g/mole
First we have to calculate the moles of  and
 and  by using ideal gas equation.
 by using ideal gas equation.
For  :
 :



For  :
 :



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

From the balanced reaction we conclude that
As, 1 mole of  react with 1 mole of
 react with 1 mole of 
So, 611.34 mole of  react with 611.34 mole of
 react with 611.34 mole of 
From this we conclude that,  is an excess reagent because the given moles are greater than the required moles and
 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.
 is a limiting reagent and it limits the formation of product.
Now we have to calculate the moles of  .
.
As, 1 mole of  react to give 1 mole of
 react to give 1 mole of 
As, 611.34 mole of  react to give 611.34 mole of
 react to give 611.34 mole of 
Now we have to calculate the mass of  .
.


The theoretical yield of  = 18340.2 g
 = 18340.2 g
The actual yield of  = 14.0 kg = 14000 g      (1 kg = 1000 g)
 = 14.0 kg = 14000 g      (1 kg = 1000 g)
Now we have to calculate the percent yield of 

Therefore, the percent yield of the reaction is, 76.34 %