WorksheetsStoichiometry Review
Total questions: 40
Worksheet time: 1hrs 1mins
The coefficients of a balanced equation indicate the relative _____of reactants and products.
masses in grams
number of moles
number of liters
densities
All stoichiometric calculations begin with a(n)_____.
skeleton equation
chemical prediction
balanced equation
actual yield
Only ____ and _____ are conserved in every reaction.
mass and volume
moles and particles
mass and number of atoms
number of atoms and volume
In order to solve stoichiometry problems, the original quantity must be expressed in _____ before calculating a value for a different material in the equation.
grams
moles
liters
it does not matter
In order for volumes to remain conserved in a chemical reaction, the products and reactants must be ______ at STP.
solids
liquids
gases
it doesn't matter--volume is always conserved.
The coefficients in a balanced equation can be used to form _____ .
conversion factors
mole ratios
volume calcuations
mass ratios
To calculate the mass of a molecule in grams, you can use ______.
the molar mass
Avogadro's number
the density at STP
the mole ratio
What is the mole ratio of A2 to B2 in the following equation?
2 A2 + B2 --> 2 A2B
2: 2
1:2
2:1
1:1
Avogadro's number
stoichiometry
product
coefficient
6.02 x 1023
0 Celsius, 1 atmosphere of pressure
the calculations of quantities in chemical reactions
stoichiometry
product
coefficient
6.02 x 1023
0 Celsius, 1 atmosphere of pressure
STP
stoichiometry
product
coefficient
6.02 x 1023
0 Celsius, 1 atmosphere of pressure
a substance formed in a chemical reaction
stoichiometry
product
coefficient
6.02 x 1023
0 Celsius, 1 atmosphere of pressure
gives the relative number of molecules, atoms or moles involved in a reaction
stoichiometry
product
coefficient
6.02 x 1023
0 Celsius, 1 atmosphere of pressure
How many moles of nitrogen are required to make 8 moles of N2O3?
2N2 + 3O2 --> 2N2O3
2
3
8
4
How many molecules of oxygen are required to make 8 molecules of N2O3?
2N2 + 3O2 --> 2N2O3
24
8
12
16
How many moles of chlorine gas will be required to react with sufficient iron to produce 7 moles of iron (III) chloride?
2 Fe(s) + 3 Cl2(g) --> 2 FeCl3(g)?
21
10.5
42
82
the starting materials in a chemical reaction
mole ratio
reactants
theoretical yield
mole
a conversion factor derived from the coefficients of a balanced chemical equation interpreted in terms of moles
mole ratio
reactants
theoretical yield
mole
the maximum amount of product that could be formed in a reaction
mole ratio
reactants
theoretical yield
mole
the amount of a substance that contains 6.02 x 1023 representative particles of a substance
mole ratio
reactants
theoretical yield
mole
the substance completely used up in a chemical reaction
limiting reagent
percent yield
actual yield
excess reagent
the ratio of how much product is produced compared to how much is expected, expressed as a percentage
limiting reagent
percent yield
actual yield
excess reagent
the amount of a product that is actually produced in a chemical reaction
limiting reagent
percent yield
actual yield
excess reagent
the substance that is left over after a reaction takes place
limiting reagent
percent yield
actual yield
excess reagent
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
What is the first thing you must do to solve a stoichiometry problem?
Make sure the chemical reaction is Balanced
Panic
Make sure the Equation is Unbalanced
Multiple by Avogadro's Number
How many moles of H2 are needed to react with 2 moles of N2 according to the reaction?
1 N2 + 3 H2 → 2 NH3
6
2
3
1
How many moles of H2O can be produced if 8 moles of H2 are reacted according to the following reaction?
2 H2 + 1 O2 → 2 H2O
4 moles
8 moles
16 moles
2 moles
How many LITERS of CO2 are produced from the combustion of 110 g of CH4 according to the reaction?
1 CH4 + 2 O2 → 1 CO2 + 2 H2O
306.9 Liters
61.6 Liters
136.9 Liters
153.4 Liters
12.00 moles of NaClO3 will produce how many grams of O2?
The theoretical yield in a reaction is 34.7g. In the lab, 29.8g of the substance is collected. What is the percentage yield?
85.87
0.8587
85.9
0.859
The theoretical yield in a reaction is 34.7g. In the lab, 29.8g of the substance is collected. What is the percentage yield?
85.87
0.8587
85.9
0.859
The percentage yield in an experiment was 97.6%. If the theoretical yield was 23.7g what was the actual yield?
24.3g
23.1g
23.1%
24.3%
What is the limiting reactant when 20g CH4 react with 15g H2O?
If 7.62g Fe react with 8.67g S, what is the limiting reactant?
