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Date
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Chemistry Unit 10 - Pre-Stoichiometry
Reviewing the Mole and Balancing Chemical Equations
Conversion Review:
*To convert from grams to moles or from moles to grams – use the periodic table and
molar mass.
*To convert from moles to particles or particles to moles – use Avogadro’s number
For example:
1 mole Na = 23 grams
1 mole NaCl = 58.5 grams
1 mole Na = 6.02 x 1023 atoms of Na
1 mole H2O = 6.02 x 1023 molecules of H2O
Molar Mass Calculations: Show all work for calculations. (Unit 8)
1. 1 mole of carbon dioxide = _____________ g of carbon dioxide
2. 1 mole of potassium chloride = _______________ g of potassium chloride
3. 1 mole of sodium phosphate = __________________ g of sodium phosphate
4. 35.75 g copper (II) chloride = ___________________ mol of copper (II) chloride
5. 175 g of aluminum oxide = ____________________ mol of aluminum oxide
6. 2.75 mol dinitrogen tetrahydride = ________________ g of dinitrogen tetrahydride
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U10 Mol Rev v2.0
Moles to Molecules and Mass to Atoms Calculations: Show all work for
calculations.(Unit 8)
1. 10.0 moles of carbon dioxide = ____________________ molecules of carbon dioxide.
2. 2.00 moles of methane (CH4) = ___________________ molecules of methane
3. 25.0 g of aluminum = __________________ atoms of aluminum
4. 5.15 x 1015 atoms of neon = _______________________ grams of neon.
Chemical Formula to Chemical Name (Unit 7)
1.
AlP = _________________________
5. ZnBr2 = _________________________
2.
FeO = _________________________
6. Ag2O = __________________________
3.
Cu(NO3)2 = ____________________
7. SiF4
4.
Fe2O3=_________________________
8. P3O5 = ___________________________
= __________________________
Chemical Name to Chemical Formula
1. copper (II) sulfite _________________ 4. aluminum hydroxide ________________
2. trihydrogen phosphate ______________ 5. chlorine gas
_________________
3. magnesium ________________________ 6. chromium (III) chloride ______________
4. nitrogen trichloride ______________
Modeling Chemistry
8. magnesium phosphate ________________
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U10 Mol Rev v2.0
Write balanced chemical equations for the following reactions.
Also, identify the reaction type of each reaction. (Unit 9) Use your
periodic table and make sure the chemical formulas are correct!
1. Lead (II) carbonate reacts with nitric acid to form lead (II) nitrate and hydrogen
carbonate.
2. Hydrogen peroxide (H2O2) reacts when exposed to sunlight to produce liquid water
and oxygen gas.
3. Magnesium chlorate is strongly heated to form magnesium chloride and oxygen gas.
4. Sodium sulfide reacts with nickel (II) nitrate to form nickel (II) sulfide and sodium
nitrate.
5. Aluminum, when hot enough, burns in air to form aluminum oxide.
6. Octane, C8H18, burns in air to produce carbon dioxide and water.
7. Solutions of sodium carbonate and iron(III) chloride react to form solid iron(III)
carbonate and sodium chloride in solution.
8. Bubbling chlorine gas through a solution of potassium iodide produces potassium
chloride and iodine.
9. Solid silver oxide can be heated and decomposed to produce silver metal and oxygen
gas.
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U10 Mol Rev v2.0
10. Ammonia (NH3) gas is bubbled through distilled water to produce ammonium
hydroxide.
11. Carbon reacts with chlorine gas to produce carbon tetrachloride.
12. Nitric acid (HNO3) reacts with barium hydroxide to produce barium nitrate and
water.
13. Calcium sulfite decomposes when heated to form calcium oxide and sulfur dioxide.
Modeling Chemistry
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U10 Mol Rev v2.0