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StoichiometryPart 1: moles to moles
IntroductionStoichiometry 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.
IntroductionStoichiometry 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.
IntroductionStoichiometry 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.
Let’s do an example.
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:
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)
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.
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)
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)
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)
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)
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)
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)
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)
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
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 ?
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 ?
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 ?
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 ?
1
Step 1: Calculate the mole ratio between CO2 and LiOH.
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 ?
1
Step 1: Calculate the mole ratio between CO2 and LiOH.
nLiOH/nCO2 = coeffLiOH/coeffCO2
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 ?
1
Step 1: Calculate the mole ratio between CO2 and LiOH.
nLiOH/nCO2 = coeffLiOH/coeffCO2 ⇒ nLiOH = (nCO2)(coeffLiOH)/coeffCO2
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 ?
1
Step 1: Calculate the mole ratio between CO2 and LiOH.
nLiOH/nCO2 = coeffLiOH/coeffCO2 ⇒ nLiOH = (nCO2)(coeffLiOH)/coeffCO2
⇒ nLiOH = (20 mol)(2)/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 ?
1
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
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
1
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
