Chemistry Worksheet 2

Predicting Reaction Products
Predict the products for the following reactions, balance the equation, then classify the type of
reaction.
1) ____ Na + ____ FeBr3 
2) ____ NaOH + ____ H2SO4 
3) ____ C2H4O2 + ____ O2 
4) ____ NH3 + ____ H2O 
5) ____ PbSO4 + _____ AgNO3 
6) ____ PBr3 
7) ____ HBr + ____ Fe 
8) ____ KMnO4 + ____ ZnCl2 
9) ____ MnO2 + ____ Sn(OH)4 
10) ____ O2 + ____ C4H10O 
11) ____ PtCl4 + ____ Cl2 
Write a balanced chemical equation for each of the following word equations below
1) aqueous barium nitrate reacts with sulfuric acid [H2SO4(aq)] to yield a barium sulfate
precipitate and nitric acid [HNO3(aq)]
2) silver nitrate reacts in solution with potassium chromate to yield a silver chromate
precipitate and soluble potassium nitrate
3) solid calcium carbonate reacts with hydrochloric acid [HCl(aq)] to yield aqueous calcium
chloride, carbon dioxide gas, and liquid water
4) aqueous zinc chloride reacts with dihydrogen monosulfide gas to yield a zinc sulfide
precipitate and hydrochloric acid
5) magnesium nitrate reacts in solution with potassium hydroxide to yield a magnesium
hydroxide precipitate and soluble potassium nitrate
For each of the following double replacement reactions, determine what the products of each
reaction will be. When you have predicted the products, balance the equation and determine
which of the products (if any) will precipitate. Assume that all reactions take place in an aqueous
solution.
1) ____ Ca(OH)2 + ____ HF 
2) ____ Pb(NO3)2 + ____ K2CrO4 
3) ____ NaC2H3O2 + ____ H2SO4 
4) ____ Cu(OH)2 + ____ H3PO4 
5) ____ AgNO3 + ____ Na2CO3 

Stoichiometry
Solve each of the following problems. Show your working and be sure to include proper units.
1. Silver and nitric acid react according to the following balanced equation:
3 Ag(s) + 4 HNO3(aq)  3 AgNO3(aq) + 2 H2O(l) + NO(g)
A. How many moles of silver are needed to react with 40 moles of nitric acid?
B. From the amount of nitric acid given in Part A, how many moles of silver nitrate will
be produced?
C. From the amount of nitric acid given in Part A, how many moles of water will be
produced?
D. From the amount of nitric acid given in Part A, how many moles of nitrogen
monoxide will be made?
2. Given the balanced equation: 2 N2H4(l) + N2O4(l)  3 N2(g) + 4 H2O(g)
A. How many moles of dinitrogen tetrahydride are required to produce 57 moles of

nitrogen?
B. How many moles of dinitrogen tetroxide are required to produce 57 moles of

nitrogen?
C. How many moles of water are produced when 57 moles of nitrogen are made?
3. Calculate the mass of aluminum oxide produced when 3.75 moles of aluminum burn in
oxygen.
4. At a very high temperature, manganese is isolated from its ore, manganomanganic oxide, via
the following balanced equation:
3 Mn3O4(s) + 8 Al(s)  4 Al2O3(s) + 9 Mn(s)
A. How many manganese atoms are liberated if 54.8 moles of Mn3O4 react with excess
aluminum.
B. How many moles of aluminum oxide are made if 3580 g of manganomanganic oxide
are consumed?
C. How many moles of manganomanganic oxide will react with 5.33 x 1025 atoms of
aluminum?
D. If 4.37 moles of aluminum are consumed, how many molecules of aluminum oxide
are produced?
5. Camels store the fat tristearin (C57H110O6) in the hump. Besides being a source of energy, the
fat is a source of water for the camel because when the fat is burned, the following
reaction occurs:
2 C57H110O6(s) + 163 O2(g)  114 CO2(g) + 110 H2O(l)
A. At STP, what volume of oxygen is required to consume 0.64 moles of tristearin?
B. At STP, what volume of carbon dioxide is produced in Part A?
C. If 22.4 L of oxygen is consumed at STP, how many moles of water are produced?
D. Find the mass of tristearin required to produce 55.56 moles of water (about 1 liter of
liquid water).
6. ___ Cu + ___ AgNO3  ___ Cu(NO3)2 + ___ Ag
How many grams of silver will be produced if 86 g of copper are used?
7. ___ (NH4)2SO4 + ___ Ca(OH)2  ___ CaSO4 + ___ NH3 + ___ H2O
At STP, how many dm3 of ammonia are produced by using 26.0 g of calcium hydroxide?
8. ___ NaCl + ___ H2SO4  ___ HCl + ___ Na2SO4
If 359 g of sodium chloride are consumed in the reaction, how many molecules of sodium
sulfate are produced?
9. ___ AgCH3COO + ___ Na3PO4  ___ Ag3PO4 + ___ NaCH3COO
What mass of AgCH3COO will react with 4.77 x 1026 molecules of sodium phosphate?
10. ___ HgO  ___ Hg + ___ O2
What mass of mercury (II) oxide is required to produce 812 liters of oxygen (at STP)?
11. ___ Ag2O  ___ Ag + ___ O2
How many molecules of silver oxide are needed to produce 445 dm3 of oxygen (at STP)?
12. ___ Al + ___ HCl  ___ AlCl3 + ___ H2
How many liters of hydrogen (at STP) are produced by reacting 3.54 x 1024 atoms of
aluminum with excess hydrochloric acid?
Limiting Reactants
Use your knowledge of stoichiometry to solve each of the following problems. Show your
working and be sure to include the proper units.
1. According to the balanced chemical equation, how many atoms of silver will be produced
from combining 100 g of copper with 200 g of silver nitrate?
Cu(s) + 2 AgNO3(aq)  Cu(NO3)2(aq) + 2 Ag(s)
2. At STP, what volume of “laughing gas” (dinitrogen monoxide) will be produced from 50 g of
nitrogen gas and 75 g of oxygen gas?
3. Carbon monoxide can be combined with hydrogen to produce methanol, CH3OH. Methanol is
used as an industrial solvent, as a reactant in some synthesis reactions, and as a clean-
burning fuel for some racing cars. If you had 152.5 kg of carbon monoxide and 24.5 kg of
hydrogen gas, how many kilograms of methanol could be produced?
4. How many grams of water will be produced from 50 g of hydrogen and 100 g of oxygen?
5. An unbalanced chemical equation is given as: ___N2H4(l) + ___N2O4(l)  ___N2(g) +

___H2O(l).
If you begin with 400 g of N2H4 and 900 g of N2O4…
A. Find the number of liters of water produced, assuming the reaction goes to
completion.
B. Find the number of liters of nitrogen produced at STP, assuming the reaction goes to
completion.
C. Find the mass of excess reactant left over at the conclusion of the reaction.
6. An unbalanced chemical equation is given as: ___Na(s) + ___O2(g)  ___Na2O(s)
If you have 100 g of sodium and 60 g of oxygen…
A. Find the number of moles of sodium oxide produced.
B. Find the mass of excess reactant left over at the conclusion of the reaction.

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Predicting Reaction Products

1) ____ Na + ____ FeBr3 

2) ____ NaOH + ____ H2SO4 

3) ____ C2H4O2 + ____ O2 

4) ____ NH3 + ____ H2O 

5) ____ PbSO4 + _____ AgNO3 

7) ____ HBr + ____ Fe 

8) ____ KMnO4 + ____ ZnCl2 

9) ____ MnO2 + ____ Sn(OH)4 

10) ____ O2 + ____ C4H10O 

11) ____ PtCl4 + ____ Cl2 

1) ____ Ca(OH)2 + ____ HF 

2) ____ Pb(NO3)2 + ____ K2CrO4 

3) ____ NaC2H3O2 + ____ H2SO4 

4) ____ Cu(OH)2 + ____ H3PO4 

5) ____ AgNO3 + ____ Na2CO3 

3 Ag(s) + 4 HNO3(aq)  3 AgNO3(aq) + 2 H2O(l) + NO(g)

2. Given the balanced equation: 2 N2H4(l) + N2O4(l)  3 N2(g) + 4 H2O(g)

A. How many moles of dinitrogen tetrahydride are required to produce 57 moles of

B. How many moles of dinitrogen tetroxide are required to produce 57 moles of

3 Mn3O4(s) + 8 Al(s)  4 Al2O3(s) + 9 Mn(s)

2 C57H110O6(s) + 163 O2(g)  114 CO2(g) + 110 H2O(l)

A. At STP, what volume of oxygen is required to consume 0.64 moles of tristearin?

B. At STP, what volume of carbon dioxide is produced in Part A?

6. ___ Cu + ___ AgNO3  ___ Cu(NO3)2 + ___ Ag

How many grams of silver will be produced if 86 g of copper are used?

8. ___ NaCl + ___ H2SO4  ___ HCl + ___ Na2SO4

10. ___ HgO  ___ Hg + ___ O2

11. ___ Ag2O  ___ Ag + ___ O2

12. ___ Al + ___ HCl  ___ AlCl3 + ___ H2

Cu(s) + 2 AgNO3(aq)  Cu(NO3)2(aq) + 2 Ag(s)

5. An unbalanced chemical equation is given as: ___N2H4(l) + ___N2O4(l)  ___N2(g) +

A. Find the number of moles of sodium oxide produced.

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1) Na + FeBr3 

2) NaOH + H2SO4 

3) C2H4O2 + O2 

4) NH3 + H2O 

5) PbSO4 + _ AgNO3 

7) HBr + Fe 

8) KMnO4 + ZnCl2 

9) MnO2 + Sn(OH)4 

10) O2 + C4H10O 

11) PtCl4 + Cl2 

1) Ca(OH)2 + HF 

2) Pb(NO3)2 + K2CrO4 

3) NaC2H3O2 + H2SO4 

4) Cu(OH)2 + H3PO4 

5) AgNO3 + Na2CO3 

6. _ Cu + _ AgNO3  _ Cu(NO3)2 + _ Ag

8. _ NaCl + _ H2SO4  _ HCl + _ Na2SO4

10. _ HgO  _ Hg + ___ O2

11. _ Ag2O  _ Ag + ___ O2

12. _ Al + _ HCl  _ AlCl3 + _ H2

5. An unbalanced chemical equation is given as: _N2H4(l) + _N2O4(l)  ___N2(g) +