Stoichiometry

1. Stoichiometry • Part 1: moles to moles

2. Introduction • Stoichiometry is the study of the mass and mole relationship between the reactants and products of a chemical reaction. • In order to do stoichiometry properly, we need to know the proper chemical equation ... • ... which means that we need to know the formulas of the reactants and products ... • ... and we need a balanced chemical equation.

3. Introduction • Stoichiometry is the study of the mass and mole relationship between the reactants and products of a chemical reaction. • In order to do stoichiometry properly, we need to know the proper chemical equation ... • ... which means that we need to know the formulas of the reactants and products ... • ... and we need a balanced chemical equation.

4. Introduction • Stoichiometry relies on the molar ratio between chemicals in the reaction. • The molar ratio is the ratio of the coefficients of the individual chemicals. • For example, in the reaction: • CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) • the molar ratio of CH4/O2 = 1/2 • This means that we need 2 moles of O2 for each 1 mole of CH4 we use.

5. Let’s do an example.

6. 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:

7. 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)

8. 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 of exhaled by a person each day.

9. 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 of exhaled by a person each day. CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l)

10. 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 of exhaled by a person each day. molar mass (g/mol) CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l)

11. 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 of exhaled by a person each day. molar mass (g/mol) 44.00 CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l)

12. 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 of exhaled by a person each day. molar mass (g/mol) 44.00 23.95 CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l)

13. 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 of exhaled by a person each day. molar mass (g/mol) 44.00 23.95 73.98 CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l)

14. 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 of exhaled by a person each day. molar mass (g/mol) 44.00 23.95 73.98 18.01 CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l)

15. 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 of exhaled by a person each day. molar mass (g/mol) 44.00 23.95 73.98 18.01 CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l) n (mol)

16. 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 of exhaled by a person each day. molar mass (g/mol) 44.00 23.95 73.98 18.01 CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l) n (mol) 20

17. 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 of exhaled by a person each day. molar mass (g/mol) 44.00 23.95 73.98 18.01 CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l) n (mol) 20 ?

18. 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 of exhaled by a person each day. molar mass (g/mol) 44.00 23.95 73.98 18.01 CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l) n (mol) 20 ?

19. 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 of exhaled by a person each day. molar mass (g/mol) 44.00 23.95 73.98 18.01 CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l) n (mol) 20 ?

20. 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 of exhaled by a person each day. molar mass (g/mol) 44.00 23.95 73.98 18.01 CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l) n (mol) 20 ? Step 1: Calculate the mole ratio between CO2 and LiOH.

21. 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 of exhaled by a person each day. molar mass (g/mol) 44.00 23.95 73.98 18.01 CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l) n (mol) 20 ? • Step 1: Calculate the mole ratio between CO2 and LiOH. • nLiOH/nCO2 = coeffLiOH/coeffCO2

22. 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 of exhaled by a person each day. molar mass (g/mol) 44.00 23.95 73.98 18.01 CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l) n (mol) 20 ? • Step 1: Calculate the mole ratio between CO2 and LiOH. • nLiOH/nCO2 = coeffLiOH/coeffCO2 ⇒ nLiOH = (nCO2)(coeffLiOH)/coeffCO2

23. 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 of exhaled by a person each day. molar mass (g/mol) 44.00 23.95 73.98 18.01 CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l) n (mol) 20 ? • Step 1: Calculate the mole ratio between CO2 and LiOH. • nLiOH/nCO2 = coeffLiOH/coeffCO2 ⇒ nLiOH = (nCO2)(coeffLiOH)/coeffCO2 • ⇒ nLiOH = (20 mol)(2)/1

24. 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 of exhaled by a person each day. molar mass (g/mol) 44.00 23.95 73.98 18.01 CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l) n (mol) 20 ? • Step 1: Calculate the mole ratio between CO2 and LiOH. • nLiOH/nCO2 = coeffLiOH/coeffCO2 ⇒ nLiOH = (nCO2)(coeffLiOH)/coeffCO2 • ⇒ nLiOH = (20 mol)(2)/1 = 40 mol

25. 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 of exhaled by a person each day. molar mass (g/mol) 44.00 23.95 73.98 18.01 CO2(g) + 2LiOH(s) → Li2CO3(s) + H2O(l) n (mol) 20 40 • Step 1: Calculate the mole ratio between CO2 and LiOH. • nLiOH/nCO2 = coeffLiOH/coeffCO2 ⇒ nLiOH = (nCO2)(coeffLiOH)/coeffCO2 • ⇒ nLiOH = (20 mol)(2)/1 = 40 mol