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Stoichiometric Calculations
The coefficients in the balanced equation give the
ratio of moles of reactants and products
Stoichiometric Calculations
From the mass of
Substance A you can
use the ratio of the
coefficients of A and B
to calculate...
Stoichiometric Calculations
Starting with 1.00 g of C6H12O6…
we calculate the moles of C6H12O6…
use the coefficients to fi...
Sample #1
• CH4 +2O2 2H2O + CO2
How many moles of CH4 are needed to make 13
moles of water?
Sample #2
• CH4 +2O2 2H2O + CO2
• How many moles of water are made from 10g
of Oxygen?
Sample #3
CH4 +2O2 2H2O + CO2
• How many grams of water are produced from
100 moles of CH4?
Sample #4
CH4 +2O2 2H2O + CO2
• How many grams of Oxygen are needed in
order to produce 200 g of carbon dioxide?
Limiting Reactants
The limiting reactant
is the reactant present
in the smallest
stoichiometric amount
Limiting Reactants
• The limiting reactant is the reactant present in the
smallest stoichiometric amount
– In other words,...
Limiting Reactants
In the example below, the O2 would be the excess
reagent
Theoretical Yield
• The theoretical yield is the amount of product
that can be made
– In other words it’s the amount of pr...
Percent Yield
A comparison of the amount actually
obtained to the amount it was possible to
make
Actual Yield
Theoretical ...
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Stoichiometric calculations

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Transcript of "Stoichiometric calculations"

  1. 1. Stoichiometric Calculations The coefficients in the balanced equation give the ratio of moles of reactants and products
  2. 2. Stoichiometric Calculations From the mass of Substance A you can use the ratio of the coefficients of A and B to calculate the mass of Substance B formed (if it’s a product) or used (if it’s a reactant)
  3. 3. Stoichiometric Calculations Starting with 1.00 g of C6H12O6… we calculate the moles of C6H12O6… use the coefficients to find the moles of H2O… and then turn the moles of water to grams C6H12O6 + 6 O2  6 CO2 + 6 H2O
  4. 4. Sample #1 • CH4 +2O2 2H2O + CO2 How many moles of CH4 are needed to make 13 moles of water?
  5. 5. Sample #2 • CH4 +2O2 2H2O + CO2 • How many moles of water are made from 10g of Oxygen?
  6. 6. Sample #3 CH4 +2O2 2H2O + CO2 • How many grams of water are produced from 100 moles of CH4?
  7. 7. Sample #4 CH4 +2O2 2H2O + CO2 • How many grams of Oxygen are needed in order to produce 200 g of carbon dioxide?
  8. 8. Limiting Reactants The limiting reactant is the reactant present in the smallest stoichiometric amount
  9. 9. Limiting Reactants • The limiting reactant is the reactant present in the smallest stoichiometric amount – In other words, it’s the reactant you’ll run out of first (in this case, the H2)
  10. 10. Limiting Reactants In the example below, the O2 would be the excess reagent
  11. 11. Theoretical Yield • The theoretical yield is the amount of product that can be made – In other words it’s the amount of product possible as calculated through the stoichiometry problem • This is different from the actual yield, the amount one actually produces and measures
  12. 12. Percent Yield A comparison of the amount actually obtained to the amount it was possible to make Actual Yield Theoretical Yield Percent Yield = x 100
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