How can amount of product (KNO₃) be predicted from amounts for two reactants (KCl, HNO₃)?

How many kilograms of potassium nitrate will be produced from 50.0 kg of potassium chloride and 50.0 kg of nitric acid in the following reaction?

4KCl + 4HNO3 + O2

4KNO3 + 2Cl2 + 2 H20

Michael Feldman

Whenever you have the amount of both reactants, you have a limiting reactant problem. For example, if I have 10 slices of bread and 10 slices of swiss cheese, I can make 5 sandwiches at most (I insist that a sandwich must have 2 slices of bread and at least one slice of cheese.) The amount of bread I have limits the amount of product I get.

You'll need 4 moles of KCl for every 4 moles of nitric acid, or some of your starting materials will be wasted. The reactant that is present in the smallest molar amount will limit the amount of product you get. So your overall strategy is to find which reactant (the KCl or nitric acid) gives you the lowest yield of potassium nitrate. That's the amount of potassium nitrate you'll actually get.

In a little more detail, the plan is to:

1. Find how many kilograms of KNO₃ you get from 50 kg of KCl. You need to convert an amount of one substance (KCl) into an amount of another (KNO₃, so you need a mole-to-mole conversion factor to bridge the two amounts. From the equation, you have 4 mol KCl = 4 mol KNO₃. The strategy is

   50 kg KCl

   formula wt. KCl

   mol KCl

   4 mol KCl = 4 mol KNO3

   mol KNO3

   formula wt. KNO3

   kg KNO3

   and the actual setup for this part of the problem is

   50 kg KCl

   (

   1000 g KCl 1 kg KCl

   )

   (

   1 mol KCl 74.55 g KCl

   )

   (

   4 mol KNO3 4 mol KCl

   )

   (

   101.11 g KNO3 1 mol KNO3

   )

   (

   1 kg KNO3 1000 g KNO3

   )

2. Find how many kilograms of KNO₃ you get from 50 kg of nitric acid. This calculation is very similar to the one in the previous step.
3. Report the lower of the two predictions as your theoretical yield of KNO₃. The reactant that limits the amount of product (the "limiting reactant") will be completely consumed in the reaction. There will be some of the other reactant left over after the reaction (which will contaminate the product).

Author: Fred Senese senese@antoine.frostburg.edu

Copyright © 1997-2001 by Fred Senese
Comments & questions to senese@antoine.frostburg.edu
Last Revised 02/23/18.URL: http://antoine.frostburg.edu/chem/senese/101-hidden/moles/faq/limiting-reagent-kcl-kno3.shtml