Download 1. You should review balancing equations and identifying types of

1. You should review balancing equations and identifying types of reactions from the
worksheets. In addition you should be able to write balanced chemical equations for reactions.
Try to write, balance, and identify the types of the following reactions:
a. the decomposition of ammonium nitrate to nitrogen gas, oxygen gas, and water vapor
2𝑁𝐻4 𝑁𝑂3 → 2𝑁2 + 𝑂2 + 4H2O
b. the reaction of sodium bicarbonate with sulfuric acid to produce sodium sulfate, water,
and carbon dioxide
2NaHCO3 +2H2SO4 Na2SO4 + 2H2O+ 2CO2
c. the treatment of phosphorus pentachloride with water to produce phosphoric acid and
hydrogen chloride
PCl5 + 4H2O  H3PO4 +5HCl
2. You should be able to set up and solve stoichiometry problems.
If the maximum amount of product possible is formed in the following reactions, what mass of
the specific product would you obtain?
a. 10 grams of sodium chloride is treated with excess silver nitrate to produce silver
chloride and sodium nitrate; How much silver chloride is precipitated? (What kind of reaction is
this?)
NaCl + AgNO3  AgCl + NaNO3
1 𝑚𝑜𝑙 𝑁𝑎𝐶𝑙
1 𝐴𝑔𝐶𝑙
10 grams X 58.5 𝑔 𝑁𝑎𝐶𝑙X
1𝑁𝑎𝐶𝑙
142.3 𝑔 𝐴𝑔𝐶𝑙
X
1 𝑚𝑜𝑙
= 24.3 g AgCl
b. 12 grams of nickel metal is treated with excess nitric acid to produce nickel (II) nitrate
and hydrogen gas; how much hydrogen gas is produced?
Ni + 2HNO3  Ni(NO3)2 + H2
1 𝑚𝑜𝑙 𝑁𝑖 1 𝐻2
2 𝑔𝐻2
12 g Ni x
x
x
= 0.41 g H2
58.7 𝑔 𝑁𝑖
1 𝑁𝑖
1 𝑚𝑜𝑙 𝐻2
c. 60 grams propane (C3H8) gas is burned in excess oxygen producing carbon dioxide
and water; how much water is produced? (What kind of reaction is this?)
Combustion
C3H8 + 5O2  3CO2 + 4H2O
60 g C3H8 X
1 𝑚𝑜𝑙 C3H8
44 𝑔 C3H8
4 𝐻2𝑂
X
18𝑔 𝐻2𝑂
X
1 C3H8 1 𝑚𝑜𝑙 𝐻2𝑂
= 98
g H2O
3. You should be able to solve limiting reactant problems.
a. Hydrazine (N2H4) reacts with dinitrogen tetroxide according to the equation:
2N2H4 (g) + N2O4 (g)  3N2 (g) + 4H2O (g)
b. 50.0 grams of hydrazine is mixed with 100.0 grams of dinitrogen tetroxide. How much
nitrogen gas was produced?
50 grams N2H4 x
1 𝑚𝑜𝑙 𝑁2𝐻4
100 grams N2O4 x
3 𝑁2
x
28𝑔 𝑁2
= 65.6 g N2 Limiting
x
32 𝑔 𝑁2𝐻4 2𝑁2𝐻4 1 𝑚𝑜𝑙
1 𝑚𝑜𝑙 𝑁2𝑂4 3 𝑁2 28𝑔 𝑁2
92 𝑔 𝑁2𝑂4
x
x
1 𝑁2𝑂4 1 𝑚𝑜𝑙
=91.3 grams N2
c. The reaction of hydrogen iodide and potassium bicarbonate produces potassium iodide
according to the equation: HI (aq) + KHCO3 (s)  KI (aq) + H2O + CO2(g)
If 32 grams of potassium bicarbonate is treated with 48 grams of hydrogen iodide, what is the
maximum amount of potassium iodide that can be produced?
1 𝑚𝑜𝑙 𝐾𝐻𝐶𝑂3
1 𝐾𝐼
166 𝑔 𝐾𝐼
32 g KHCO3 x 100 𝑔 𝐾𝐻𝐶𝑂3x 1 𝐾𝐻𝐶𝑂3x 1 𝑚𝑜𝑙 𝐾𝐼= 53 g KI limiting
1 𝐻𝐼
1 𝐾𝐼
166 𝑔 𝐾𝐼
48 g HI x 128 𝑔 𝐻𝐼x 1 𝐻𝐼x 1 𝑚𝑜𝑙 𝐾𝐼= 62 g KI
d. TNT (trinitrotoluene) is prepared by treating toluene with nitric acid according to the
equation: C7H8 (l) + 3HNO3 (aq)  C7H5(NO2)3 (s) + 3H2O (l)
What mass of TNT (C7H8(NO2)3) can be made when 450 grams of toluene (C7H8) is treated with
1000 grams of nitric acid?
450 grams toluene
1 𝑚𝑜𝑙 𝑡𝑜𝑙𝑢𝑒𝑛𝑒
92 𝑔 𝑡𝑜𝑙𝑢𝑒𝑛𝑒
1000 grams HNO3 x
1 𝑇𝑁𝑇
1 𝑚𝑜𝑙 𝐻𝑁𝑂3
63 𝑔 𝐻𝑁𝑂3
227 𝑔 𝑇𝑁𝑇
x 1 𝑡𝑜𝑙𝑢𝑒𝑛𝑒x 1 𝑚𝑜𝑙 𝑇𝑁𝑇= 1110 grams TNT limiting
1 𝑇𝑁𝑇
x 3 𝐻𝑁𝑂3x 450 grams TNT= 2381 grams TNT
4. You should be able to set up and solve percent yield problems.
Nitrous oxide reacts with oxygen to produce nitrogen dioxide according to the equation:
2N2O (g) + 3O2 (g)  4NO2 (g)
a. What mass of nitrogen dioxide can be made from 42 grams of nitrous oxide and 42 grams of
oxygen?
42 grams N2O x
42 grams O2 x
1 𝑚𝑜𝑙 𝑁2𝑂
44 𝑔 𝑁20
1 𝑚𝑜𝑙 𝑂2
32 𝑔 𝑂2
x
4𝑁𝑂2
46 𝑔 𝑁𝑂2
2𝑁2𝑂
1 𝑚𝑜𝑙
3 𝑂2
x 2 𝑁20x
x
= 87.8 grams NO2
46 𝑔 𝑁𝑂2
1 𝑚𝑜𝑙
= 90.5 grams O2
b. If only 75 grams of nitrogen dioxide was produced in the reaction described in the previous
questions, what was the % yield?
75 𝑔𝑟𝑎𝑚𝑠 𝑁𝑂2
x 100= 85.4 % yield
87.8 𝑔𝑟𝑎𝑚𝑠 𝑁𝑂2