Chapter 9 stoich
Transcript of Chapter 9 stoich
Chapter 9- Stoichiometry:
• Stoichiometry is like following a recipe
• Focuses on mass or molar relationships
• Key is a balanced equation and reading the equation in terms of…Coefficients
I have a yellow hat on!
The mass relationships between reactants and products in a chemical reaction.
Let’s try this:
1. Type of reaction?
2. Balanced equation
3. How is this read in terms of moles?
4. What are all the possible mole ratios?
5. “RECIPE” for moles to moles, moles to mass, mass to moles and mass to mass
Na + Cl2
Let’s try this:
1. Type of reaction?
2. Balanced equation
3. How is this read in terms of moles?
4. What are all the possible mole ratios?
5. “RECIPE” for moles to moles, moles to mass, mass to moles and mass to mass
Na + Cl2 NaCl
Let’s try this:
1. Type of reaction? Synthesis
2. Balanced equation
3. How is this read in terms of moles?
4. What are all the possible mole ratios?
5. “RECIPE” for moles to moles, moles to mass, mass to moles and mass to mass
Na + Cl2 NaCl
Let’s try this:
1. Type of reaction? Synthesis
2. Balanced equation
3. How is this read in terms of moles?
4. What are all the possible mole ratios?
5. “RECIPE” for moles to moles, moles to mass, mass to moles and mass to mass
2Na + Cl2 2NaCl
Let’s try this:
1. Type of reaction? Synthesis
2. Balanced equation
3. How is this read in terms of moles?
2 moles of Na react with 1 mole of Cl2 to produce 2 moles of NaCl
2Na + Cl2 2NaCl
Let’s try this:
1. What are all the possible mole ratios?
2 mol Na 2 mol Na 1 mol Cl2 1 mol Cl2 2 mol NaCl 2 mol NaCl
2 mol NaCl 2 Mol NaCl 1 mol Cl2 2 mol Na 1 mol Cl2 2 mol Na
2Na + Cl2 2NaCl
Let’s try this:
5. “RECIPE” for moles to moles, moles to mass, mass to moles and mass to mass
Remember that you cannot use a mass-mass
ratio. You must convert to mol first and then
back into grams.
2Na + Cl2 2NaCl
Conversions of Quantities in Moles
CO2 + 2LiOH → Li2CO3 + H2O
How many moles of lithium hydroxide are
required to react with 20 moles of carbon
dioxide, the average amount exhaled by a
person each day?
Conversions of Quantities in Moles
CO2 + 2LiOH → Li2CO3 + H2O
Conversions of Quantities in Moles
CO2 + 2LiOH → Li2CO3 + H2O
2 mol LiOH
1 mol CO2
Conversions of Quantities in Moles
CO2 + 2LiOH → Li2CO3 + H2O
2 mol LiOH x mol LiOH
1 mol CO2 20 mol CO2
X
Conversions of Quantities in Moles
CO2 + 2LiOH → Li2CO3 + H2O
2 mol LiOH x mol LiOH
1 mol CO2 20 mol CO2
x 40 mol LiOH
X
=
More Practice
Use the following equation to determine how many grams of aluminum must be used to produce 5.00 grams of hydrogen gas?
2 Al(s) + 6 HCl(aq) 2 AlCl3(aq) + 3 H2(g)
Do Now
In the reaction P4 + 5 O2 2 P2O5, how many moles of oxygen are consumed each time 0.500 mol of P2O5 is formed?
Answer: 1.25 mol O2
Limiting ReagentLet’s pretend we have 7,000,000 hot dogs
But only 600 hot dog buns
X 1,000,000
X 100
Limiting ReagentQ- How many hot dogs can you make?
Limiting ReagentQ- How many hot dogs can you make?
A – Only 600
Limiting Reagent Once a reactant is used up, there can be no more products produced
(The substance that is used up first is called the)limiting reagent =
the reactant that limits the amount of the other reactant that can be combined and thus the
product that is produced
Excess reagent = the substance not used up completely
Let’s try a problem:
HCl + NaOH NaCl + H2O
2 mol 2.5 mol
Determine the limiting reagent for this reaction.
(This is done by comparing the 2 given value in
a ratio.)
Let’s try a problem:HCl + NaOH NaCl + H2O
2 mol 2.5 mol
Pick one of the givens and solve:
1 mol HCl x mol HCl
1 mol NaOH 2.5 mol NaOH
x 2.5 mol HCl
=
=
Let’s try a problem:HCl + NaOH NaCl + H2O
2 mol 2.5 mol
2.5 mol HCl: But what does this mean?
This means that in order to react ALL
2.5 mol NaOH, you would need AT LEAST
2.5 mol HCL.
But you only have 2 mol HCl, so it LIMITS
the reaction. Hence: limiting reagent.
Percentage Yield• Theoretical yield = what you calculate or
expect under perfect conditions
• Actual Yield = what you get in the lab
• Percentage Yield = x 100%Actual Yield
Theoretical Yield