1. Section 9-2: Ideal Stoichiometric Calculations
Coach Kelsoe
Chemistry
Pages 304–311

2. Section 9-2 Objectives
Calculate the amount in moles of a reactant or product from the amount in moles of a different reactant or product.
Calculate the mass of a reactant or product from the amount in moles of a different reactant or product.
Calculate the amount in moles of a reactant or product from the mass of a different reactant or product.
Calculate the mass of a reactant or product from the mass of a different reactant or product.

3. Ideal Stoichiometric Calculations
The chemical equation plays a very important part in all stoichiometric calculations because the mole ratio is obtained directly from it. Solving any reaction-stoichiometry problem must begin with a balanced equation.
Chemical equations help us make predictions about chemical reactions without having to run the reactions in the laboratory.
The calculations we make in this section are THEORETICAL. They tell us the amounts of reactants and products under ideal conditions.

4. Ideal Stoichiometric Calculations
Ideal conditions are rarely met in the lab or in industry. Yet, theoretical stoichiometric calculations serve the very important function of showing the maximum amount of product that could be obtained before a reaction is run in the laboratory.
Solving stoichiometric problems requires practice. Use a logical and systematic approach along with your previous knowledge of chemistry to work through these problems.

5. Conversions of Quantities in Moles
In these stoichiometric problems, you are asked to calculate the amount in moles of one substance that will react with or be produced from the given amount in moles of another substance.
The plan for a simple mole conversion problem is: Amount of Amount of given unknown substance (in mol) substance (in mol)

6. Conversions of Quantities in Moles
These type of problems require only one conversion factor: the mole ratio of the unknown substance to the given substance from the balanced equation.
given quantity x conversion factor = unknown quantity

7. Sample Problem 9-1
In a spacecraft, the carbon dioxide exhaled by astronauts can be removed by its reaction with lithium hydroxide, LiOH, according to the following chemical equation: CO2(g) + 2LiOH(s)  Li2CO3(s) + H2O(l)
How many moles of lithium hydroxide are required to react with 20 mol of CO2, the average amount exhaled by a person each day?

8. Sample Problem 9-1
Given: amount of CO2 = 20 mol; formula- CO2(g) + 2LiOH(s)  Li2CO3(s) + H2O(l)
Unknown: amount of LiOH in moles
Answer: 20 mol CO2 x 2 mol LiOH = 40 mol LiOH
1 mol CO2

9. Sample Problem
Ammonia, NH3, is widely used as a fertilizer and in many household cleaners. How many moles of ammonia are produced when 6 mol of hydrogen gas react with an excess of nitrogen gas?
Given: moles of hydrogen gas, H2,= 6 mol
Unknown: moles of ammonia, formula

10. Sample Answer N2 + H2  NH3 (unbalanced) N2 + 3H2  2NH3 (balanced)
6.0 mol H2 x 2 mol NH3 = 4.0 mol NH3
3 mol H2

11. Conversions of Amounts in Moles to Mass
In the following calculations, you will be asked to calculate the mass of a substance that will react with or be produced from a given amount in moles of a second substance.
This plan requires two conversion factors: mole ratio of the unknown and given substances and the molar mass of the unknown substance.

12. Conversions of Amounts in Moles to Mass
Amount of Amount of Mass of given unknown unknown substance substance substance (in mol) (in mol) (in grams)

13. Sample Problem 9-2
In photosynthesis, plants use energy from the sun to produce glucose, C6H12O6, and oxygen from the reaction of carbon dioxide and water. What mass, in grams, of glucose is produced when 3.00 mol of water react with carbon dioxide?
Given: moles of water, H2O, = 3.00 mol
Unknown: balanced chemical equation, mass of glucose

14. Sample Problem 9-2 CO2 + H2O  C6H12O6 + O2 (unbalanced)
6CO2 + 6H2O  C6H12O6 + 6O2 (balanced)
3.00 mol H2O x 1 mol C6H12O6 x g C6H12O6 = 90.1 g
6 mol H2O
6 mol C6H12O6

15. Sample Problem
What mass of carbon dioxide, in grams, is needed to react with 3.00 mol of H2O in the photosynthetic reaction described in the last problem?
Given: moles of water, H2O, = 3.00 mol
Unknown: balanced chemical equation, mass of carbon dioxide

16. Sample Problem CO2 + H2O  C6H12O6 + O2 (unbalanced)
6CO2 + 6H2O  C6H12O6 + 6O2 (balanced)
3.00 mol H2O x 6 mol CO2 x g CO2 = 132 g
6 mol H2O
1 mol CO2

17. Conversions of Mass to Amounts in Moles
In these problems, you start with a mass and converting that mass to moles, then using another conversion factor to convert from your given substance to your unknown substance.
Mass of Amount of Amount of given given unknown substance substance substance (in grams) (in mol) (in mol)

18. Sample Problem 9-3
The first step in the industrial manufacture of nitric acid is the catalytic oxidation of ammonia. NH3(g) + O2(g)  NO(g) + H2O(g) The reaction is run using 824 g of NH3 and excess oxygen. How many moles of H2O are formed?
Given: mass of ammonia, NH3 = 824 g
Unknown: balanced chemical equation, moles of H2O

19. Sample Problem 9-3 NH3 + O2  NO + H2O (unbalanced)
4NH3 + 5O2  4NO + 6H2O (balanced)
824 g NH3 x 1 mol NH3 x 6 mol H2O = 72.6 mol
17.04 g NH3
4 mol NH3

20. Mass-Mass Calculations
Mass-mass calculations are more practical than other mole calculations we’ve studied.
You can never measure moles directly. You are generally required to calculate the amount in moles of a substance from its mass, which you can measure in the lab.
Mass-mass problems can be viewed as the combination of the other types of problems.

21. Mass-Mass Calculations
Mass of Amount of Amount of Mass of given given unknown unknown substance substance substance substance (in grams) (in mol) (in mol) (in grams)

22. Sample Problem 9-4
Tin(II) fluoride, SnF2, is used in some toothpastes. It is made by the reaction of tin with hydrogen fluoride according to the following equation Sn(s) + 2HF  SnF2(s) + H2(g) How many grams of SnF2 are produced from the reaction of g of HF with Sn?
Given: mass of HF, balanced equation
Unknown: mass of SnF2

23. Sample Problem 9-4 Step 1: Convert grams of given to moles of given.
Step 2: Convert moles of given to moles of unknown.
Step 3: Convert moles of unknown to grams of unknown.
30.00 g HF x 1 mol HF x 1 mol SnF2 x g SnF2 = g
20.01 g HF
2 mol HF
1 mol SnF2