Download W2(SO4)3 + Mg3(PO4)2 --------> WPO4 + MgSO4

The Arts Academy at Benjamin Rush
Chemistry – Mr. Wagenhoffer
Balancing Reactions Bonus Credit
Name:_____________________________________________________________________________________ Date:__________________________
For the following reactions, simply balance them.
Odd/Even Technique:
N2 + H2 -----> NH3
Al + O2 ------> Al2O3
P + Br2 -------> PBr3
N2 + F2 --------> NF3
B + Cl2 -------> BCl3
Inspection Method
Na2SO4 + BaCl2 -------> NaCl + BaSO4
H2CO3 + KOH --------> HOH + K2CO3
Fe(OH)3 + Na3PO4 ------> FePO4 + NaOH
W2(SO4)3 + Mg3(PO4)2 --------> WPO4 + MgSO4
K3AsO4 + AlBr3 --------> KBr + AlAsO4
Balancing from the Largest Compound First
AlBr3 + H2SO4 -------> HBr + Al2(SO4)3
Ba(OH)2 + H3PO4 -------> Ba3(PO4)2 + HOH
K2SO4 + BF3 --------> B2(SO4)3 + KF
MgBr2 + Na3PO4 --------> Mg3(PO4)2 + NaBr
Combustion Balancing – C, H, O
CH4 + O2 --------> CO2 + H2O
C2H6 + O2 --------> CO2 + H2O
C3H8 + O2 --------> CO2 + H2O
C4H10 + O2 --------> CO2 + H2O
C5H12 + O2 --------> CO2 + H2O
Assorted Balancing (in no particular order)
a.
ZnBr2 + Na2SO4 ------------> ZnSO4 + NaBr
b.
C2H3O2 + O2 --------------> CO2 + H2O
c.
Ra + H2O ------------> RaOH + H2
d.
Mg + O2 ------------> MgO
e.
Na2O -------------> Na + O2
f.
FeS + HCl -------------> FeCl2 + H2S
g.
AgNO3 + NaCl --------------> AgCl + NaNO3
h.
Fe + CuNO3 ------------------> Fe(NO3)2 + Cu
i.
H2 + O2 -------------------> H2O
j.
Ca(OH)2 + KF ------------------> CaF2 + KOH
k.
Zn + H2CO3 ------------------> Zn2 (CO3)3 + H2
l.
C8H18 + O2 ------------------> CO2 + H2O
m. FeSO4 + H2O -------------------> Fe(OH)2 + H2SO4
n.
ZnO2 + AgNO3 ---------------------------> Zn (NO3)4 + Ag2O
The Arts Academy at Benjamin Rush
Chemistry – Mr. Wagenhoffer
Predicting Reactions Bonus
Name:_______________________________________________________________________________ Date:________________________________
The Five Basic Types of Reactions
Match the following reaction type with its correct basic formula
a) Synthesis
b) Decomposition
c) Combustion
d) Single Replacement
e) Double Displacement
1) A + BC ------> AC + B
2) A + B --------> AB
3) AB + CD ------> AD + CB
4) CxHy + O2 ------> CO2 + H2O
5) AB ---------> A + B
Identifying types of Reactions
Write the type of reaction next to the reaction provided
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
k.
l.
CaO + H2O --------------> Ca(OH)2
C12H22O11 ----------------> 12C + 11H2O
Zn + H2SO4 ---------------> ZnSO4 + H2
ZnBr2 + Na2SO4 ------------> ZnSO4 + 2NaBr
C2H3O2 + O2 --------------> CO2 + H2O
Ra + H2O ------------> RaOH + H2
Mg + O2 ------------> MgO
Na2O -------------> Na + O2
FeS + 2HCl -------------> FeCl2 + H2S
AgNO3 + NaCl --------------> AgCl + NaNO3
Fe + 2CuNO3 ------------------> Fe(NO3)2 + 2Cu
2H2 + O2 -------------------> 2H2O
To predict any reaction, be sure to…
1. Write out the reactants
2. Identify the type of reaction
3. Predict the products
4. Use the oxidation numbers to fix the subscripts for each product and reactant
5. Balance the reaction
Predicting Synthesis
Al + O2 ------->
C + O2 -------->
Mg + O2 ------->
Solid silver (+1) is placed into a container of chlorine gas
Hydrogen gas and Oxygen gas are ignited in a container.
Decomposition
H2O ----->
CaO ------->
Combustion
The combustion of methane, CH4
The combustion of propane, C3H8
The combustion of butane, C4H10
The combustion of pentane, C5H12
Single Replacement
Mg + HBr ----->
Al + H3PO4 ------>
Ca + HOH ------>
Magnesium is added to a solution of Silver (I) Nitrate
Zinc (II) is added to a solution of hydrochloric acid
Double Displacement
NaBr + CaSO4 -------->
FeBr3 + H2SO4 -------->
AlF3 + H2CO3 -------->
Solutions of sodium chloride and silver (I) nitrate are mixed together
Solutions of magnesium hydroxide and hydrobromic acid are mixed together
Assorted Reaction Predictions
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
Aluminum is mixed with Fluorine gas.
A solution of Barium Sulfate is placed into a solution of Boron Bromide.
Methane (CH4) is combusted.
Solid Silver (+1 charge) is added to a solution of Hydrochloric Acid.
Copper (+2 charge) wire is added to a solution of Silver (I) Nitrate.
A solution of sodium hydroxide is added to a solution of beryllium phosphate.
C12H36 + O2 ----------------->
Ra + I2 ------------------->
Fe3(AsO4)2 + Cu2SO3 ----------------->
Zn3+ + O2 ------------------>
The Arts Academy at Benjamin Rush
Chemistry – Mr. Wagenhoffer
Net Ionic Reaction Bonus
Name:______________________________________________________________________________________ Date:_________________________
Solubility Rules:
1.
2.
3.
4.
5.
Ag+, Pb2-, Hg22+ with group 17 elements are insoluble (form a solid in solution).
BaSO4, CaSO4, PbSO4, Hg2SO4 are insoluble (form a solid in solution).
S2-, CrO42-, CO32-, PO43- are insoluble (form a solid in a solution).
Metals on their own = solid
Diatomic elements on their own = gas
Using Solubility Rules
For the following compounds/elements, indicate their state of matter based on the solubility rules above. If
not on the rules, assume the substance is aqueous, (aq)
FeBr3
H2O
NaCl
BaSO4
LiF
AgNO3
AgCl
Br2
Al2(CrO4)3
PbCl2
PbSO4
KOH
Na2O
BaS
AlPO4
Ba3(PO4)2
Ag
Cu
O2
Mg
KBr
To predict any net ionic reaction, be sure to…
1. Write down the reactants
2. Predict the type of reaction and get the products
3. Use the oxidation numbers to get the correct subscripts for products and reactants
4. Balance the reaction
5. Use the solubility rules to predict the state of matter of each compound / element
6. Break apart any aqueous substances into their ions
7. Cancel the spectator ions (aqueous on both sides)
8. Report the net ionic reaction
Predicting solubility rules and breaking apart aqueous ions
For each example, simply provide the correct states of matter and break apart the aqueous ions. Report any
spectator ions you find.
Mg + 2HCl -----> MgCl2 + H2
Cu + AgNO3 -------> CuNO3 + Ag
BaF2 + H2SO4 ------> 2HF + BaSO4
HCl + NaOH --------> HOH + NaCl
Zn + 2HBr -------> ZnBr2 + H2
Canceling Spectators and Reporting Net Ionic Reactions
Given the following complete ionic reactions, cancel any spectators and report the net ionic reaction.
Mg (s) + 2H+ + 2Br- ------> Mg+2 + 2Br- + H2 (g)
H+ + Cl- + Na+ + OH- ------> H2O (l) + Na+ + ClMg(OH)2 (s) + 2H+ + 2F- -------> H2O (l) + Mg+2 + 2FCa+2 + 2OH- + Fe+2 + 2Cl- -------> Ca+2 + 2Cl- + Fe(OH)2 (s)
Fe (s) + 2Ag+ + 2NO3- -------> Fe+2 + 2NO3- + 2Ag (s)
Assorted Practice
Report the net ionic reaction of the following processes. Be sure to predict the states of matter and cancel any
spectator ions!
K2CO3 (aq) + MgI2 (aq) ----->
2KI +
MgCO3
2Hg(NO3) (aq) + CuSO4 (aq) -----> Hg2SO4 +
K2SO4 (aq) + Ba(OH)2 (aq) ----->
Cu (s) + AgNO3 (aq) --------->
Mg (s) + HBr (aq) ----------->
2KOH
Cu(NO3)2
+
BaSO4
Cu(NO3)2 + Ag
MgBr2
+
H2
Solutions of barium chloride and sodium sulfate are mixed.
Solutions of sodium chloride and silver (I) nitrate are mixed.
Copper wire is placed into a solution of silver (I) nitrate.
Magnesium metal is placed into a solution of sulfuric acid.
The Arts Academy at Benjamin Rush
Chemistry – Mr. Wagenhoffer
Application of the Mole Bonus
Name:_______________________________________________________________________________ Date:________________________________
Mass Percentages
For each example, you need to find the formula weight of the compound given, and find the mass percentage
for each atom in that compound. Remember, to do mass percentages, you must…
1. Find the formula weight of the entire compound
2. Find the percentage of each atom by dividing the mass of each atom in the compound by the formula
weight of the compound. Then, multiply by 100! (because it is PERCENT)
Na2SO4
BaCl2
K3PO4
Mg3(AsO4)2
Ca(OH)2
HNO3
Average Atomic Masses
For each example, you need to determine the average atomic mass (amu) for each given atom. Remember…
1. Change each percentage to their decimal equivalent
2. Multiply that decimal percent by the mass of the isotope
3. Add all of the masses together at the end to determine the amu
Iron, where…. 80.0% has a mass of 55.0 and 20.0% has a mass of 56.0
Carbon, where… 99.9% has a mass of 12.0 and 0.08% has a mass of 13.0 and 0.02% has a mass of 14.0
Bromine, where… 90.0% has a mass of 79.0 and 10.0% has a mass of 80.0
Calcium, where… 60.0% has a mass of 40.0 and 40.0% has a mass of 41.0
Empirical Formulas from Molecular Formulas
For each example, provide the empirical formula (remember, it is the simplest form).
C6H12O6
C3H6
S2O6
K4C2O6
C5H10O5N5
C6H18O4
Molecular Formulas from empirical data
For each example, provide the molecular formula given the empirical formula and the molecular formula
weight. Remember…
1. Determine the FW of the empirical formula
2. Divide the molecular FW by the empirical FW (this tells you how much larger the molecular is)
3. Multiply the empirical formula by how much larger the molecular is (from step 2)
CH3 molecular FW = 30.0 g/mol
C2H5
molecular FW = 58.0 g/mol
C2H3O2 molecular FW = 118 g/mol
NO2
molecular FW = 138.0 g/mol
Empirical Formulas from Mass Percentages
For each of the examples, determine the empirical formulas given the mass percentages. Remember to….
1. Assume 100 grams of the compound (so each mass percent is a mass of the atom)
2. Convert those atom masses into moles (mol = g/FW)
3. Divide each mole value by the smallest number (this gets you the empirical ratios)
4. If necessary, multiply each number to make it a whole number (ex: 0.5 multiplies by 2,
0.33 multiplies by 3)
A compound that is 48.0% carbon, 48% oxygen, and 4.00% hydrogen by mass.
A compound that is 60.0% carbon, 36.0% chlorine, and the rest hydrogen by mass.
A compound that is 60.0% carbon, 32.0% sulfur, and the rest oxygen by mass.
A compound that is 54.1% calcium, 2.70% hydrogen, and 43.2% oxygen by mass.
A compound that is 39.7% sodium and the rest chlorine by mass.
Assorted Practice
Given the formula: AgC2H3O2 determine the mass percent of Silver, Carbon, Hydrogen, and Oxygen.
Given the formula: Fe2(SO4)3 determine the mass percent of Iron, Sulfur, and Oxygen.
Determine the average atomic mass of Calcium given: 89.90 % Ca–40, 10.10 % Ca–41
Determine the average atomic mass of carbon given: 96.95 % C–12, 2.90 % C–14, and 0.15 % C–16.
Determine the average atomic mass of Chromium given: 83.79 % Cr–52, 9.50 % Cr–53, 4.35 % Cr–50, and
2.36 % Cr–54.
Provide the molecular formula given the formula weight of the molecular and the empirical formula.
a. CH2O, molecular formula weight: 90 g/mol
b. OH, molecular formula weight: 34 g/mol
c. P2O5, molecular formula weight: 426 g/mol
A compound is 27.0 % Na, 16.5 % N, and 56.5 % O by mass. Determine the empirical formula.
i. If the molecular FW of the above compound is 170.0 g/mol, determine the molecular formula.
NutraSweet, a common sugar substitute, is made up of 57.14% C, 6.16% H, 9.52% N, and the rest oxygen by
mass. If the molar mass of the compound is 294.30 g/mol, determine both the empirical and molecular
formulas for this compound.
The Arts Academy at Benjamin Rush
Chemistry – Mr. Wagenhoffer
Stoichiometry Bonus
Name:___________________________________________________________________________________ Date:____________________________
For each example, you must solve for each stoichiometry reaction. Remember, stoichiometry is the study of
the quantities of reactants and products in a chemical process. The key to stoichiometry is the mole ratio, the
balanced coefficients in front of each product and reactant in a given reaction. For each of the examples,
remember the following steps:
1. Each reaction must be balanced!!! (most important step!)
2. Make sure all units are converted to moles
3. Identify what you want and what you have
4. Multiply your starting moles by your mole ratio (what you want/what you have)
5. Convert the ending moles (if necessary)
Forming Mole Ratios
For the following example, use the reaction and form only the mole ratio based on the data that is given:
3Ba(OH)2 + 2H3PO4 -------> Ba3(PO4)2 + 6HOH
If you start with barium hydroxide, how much barium phosphate could you produce?
If you start with phosphoric acid, how much barium phosphate could you produce?
If you start with barium hydroxide, how much water could you produce?
If you end up with water, how many moles of phosphoric acid were necessary?
If you have moles of barium phosphate, how much barium hydroxide was necessary?
Stoichiometry with just moles
For the following example, use the reaction below to solve the problems that follow:
2KOH + H2SO4 -------> 2HOH + K2SO4
If you begin with 2.5 moles of potassium hydroxide, how many moles of water could you produce?
If you begin with 2.5 moles of sulfuric acid, how many moles of water could you produce?
If you start with 0.56 moles of sulfuric acid, how many moles of potassium sulfate could you produce?
If you start with 0.250 moles of potassium hydroxide, how many moles of water could you produce?
If you end with 0.845 moles of water, how much sulfuric acid was used?
If you end up with 0.456 moles of potassium sulfate, how much potassium hydroxide was used?
If you begin with 12.5 grams of potassium hydroxide, how many moles of water could be produced?
If you begin with 10.0 grams of sulfuric acid, how many moles of potassium sulfate could be produced?
If you begin with 45.0 grams of potassium hydroxide, how many moles of potassium sulfate form?
Assorted practice
Solve the following stoichiometric problems. MAKE SURE that each equation is BALANCED!
a.
Given the equation: Fe + KOH ------------> Fe(OH)3
+
K
find the number of moles of potassium if you begin with 9.4 moles of Iron.
b.
Given the equation:
Ag(NO3)2
+
NaCl ------------>
AgCl2
+
NaNO3
find the number of moles of Silver Chloride if you begin with 0.75 moles of Sodium Chloride.
c.
Given the equation: H2 +
Br2
----------->
HBr
find the number of grams of HBr if you begin with 4.27 moles of Hydrogen.
d.
Given the equation: H3PO4 +
MgSO4
----------->
H2SO4
+
Mg3(PO4)2
find the number of grams of H2SO4 if you begin with 3.49 moles of H3PO4.
Consider the reaction:
W2(SO4)3 + Mg3(PO4)2 -----------> 2WPO4 + 3MgSO4
You begin the reaction with 65.5 grams of Magnesium Phosphate.
a.
b.
c.
What is the formula weight of magnesium phosphate?
How many moles of magnesium phosphate do you have?
How many moles of tungsten phosphate could you produce?
Consider the reaction:
Fe + CuNO3 ------------------> Fe(NO3)2 + Cu
You begin the reaction with 28 grams of iron.
a.
b.
c.
d.
e.
f.
Balance the chemical reaction
Convert the grams of iron to moles.
How many moles of Fe(NO3)2 can you make?
How many grams of Fe(NO3)2 can you make?
How many moles of Copper could you produce?
How many grams of copper could you produce?