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Stoichiometry

Stoichiometry. Part 1: moles to moles. 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 ...

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Stoichiometry

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  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

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