Vocabulary
This term describes how much product is actually formed.
Actual yield
2 HCl + CaCO3 --> CaCl2 + H2O + CO2
If 15.00 g of CaCO3 react, what is the theoretical yield of CO2?
6.60 grams
If the theoretical yield is 6.59 grams, but the actual yield is 2.50 grams, what is the percent yield?
37.9%
The type of reactant that determines how much product you can form.
The limiting reactant
The type of reactant that forms leftovers.
The excess reactant.
What is the formula for percent yield?
2 HCl + CaCO3 --> CaCl2 + H2O + CO2
If 4.50 g of HCl react, what is the theoretical yield of CO2?
2.71 g
If the theoretical yield is 2.73 grams, and the actual yield is 2.70 grams, what is the percent yield?
99.6%
Balance the following chemical equation:
___ Al + ___ HCl --> ___AlCl3 + ____H2
2 Al + 6 HCl --> 2 AlCl3 + 3 H2
Balance the following chemical equation:
__ Cl2(g) + ___ NaI (aq) → ___ NaCl(aq) + ___ I2
Cl2(g) + 2 NaI(aq) → 2 NaCl(aq) + I2
What conversion pathway is commonly used for calculating the theoretical yield?
Gram to gram conversion pathway
P4(s) + 6 Cl2(g) --> 4 PCl3(l)
If 85.4 grams of chlorine react, how much phosphorous trichloride is formed?
110.0 grams
A reaction with a calculated yield of 9.23 g produced 7.89 g of product. What is the percent yield for this reaction?
85.5%
A reaction with Iron and Sulfur produces the following products.
When using 3.9 moles of Iron the reaction produces 4.5 moles of FeS.
When using 4.8 moles of Sulfur the reaction produces 3.9 moles of FeS.
What is the limiting reactant?
Sulfur
A reaction with Iron and Sulfur produces the following products.
When using 3.9 moles of Iron the reaction produces 4.5 moles of FeS.
When using 4.8 moles of Sulfur the reaction produces 3.9 moles of FeS.
What is the excess reactant?
Iron
DOUBLE JEOPARDY!
What are the steps of determining the amount of leftovers?
1. Use the number of moles that can be formed.
2. Determine mole ratio between product and excess reactant.
3. Subtract value from the original value in problem.
2 NH3(g) + CO2(g) --> CN2OH4(s) + H2O(l)
If 9.87 grams of NH3 react, what is the theoretical yield of CN2OH4(s)?
17.4 grams
If the theoretical yield is 110.0 grams and the actual yield is 104 grams, what is the percent yield?
94.5%
DOUBLE JEOPARDY!
Pb(NO3)2(aq) + 2 HCl(aq) → PbCl2(s) + 2 HNO3(aq)
If 15.0 g of each reactant is used, what is the limiting reactant?
Pb(NO3)2
DOUBLE JEOPARDY!!
2 Al + 6 HCl --> 2 AlCl3 + 3 H2
If 15.0 g of each reactant is used, which is the limiting reactant?
HCl
TRUE or FALSE
Limiting reactants can only be found if the problem is given in moles.
False
You can find the limiting reactant with grams as well!
2 NH3(g) + CO2(g) --> CN2OH4(s) + H2O(l)
If 5.96 grams of NH3 react, what is the theoretical yield of CN2OH4(s)?
10.5 grams
DOUBLE JEOPARDY!
CH3OH (g) --> CH2O(g) + H2(g)
15.4 g of CH3OH reacts completely according to the reaction, and only 12.35 grams of CH2O is formed, what is the percent yield?
85.8%
DOUBLE JEOPARDY!
4 FeS2 + 11 O2 → 2 Fe2O3 + 8 SO2
When 26.62 moles of FeS2 reacts with 5.44 moles of O2, how many moles of SO2 are formed?
3.96 mol SO2
DOUBLE JEOPARDY!
2 CuCl2 + 4 KI → 2 CuI + 4 KCl + I2
When 0.56 moles of CuCl2 reacts with 0.64 moles of KI, how many moles of I2 are formed?
0.160 mol I2