Things that should be in your notebook when it’s turned in…
Menu Worksheet
p.372 #3, 4
p.375#11, 12
p.387 #28, 29, 30
Stoichiometry Lab
Mass-to-Mass Worksheet
p.376 #13
p.377 #15
S’more Lab
Study Guide 5
Make sure all your work is on a separate sheet of paper. You will only get full credit if every problem is
completed. Don’t leave any blank.
For the test, you need to be able to…
…write the formulas for compounds…mainly so you get their masses and reactions correct…
1. Write the formulas for…
a) nitrogen
b) ammonia
c) hydrochloric acid
d) chromium (IV) carbonate
e) sodium
f) lead (II) chloride g) ammonium oxide
h) aluminum hydroxide
…move among moles, atoms, molecules, and grams of one substance using dimensional analysis…
2. What would the mass of 24 moles of lithium oxide be?
3. How many atoms would you find in 56.4 grams of carbon?
4. Which would have more mass – 3.2 moles of magnesium or 1.30 x 1024 molecules of oxygen
gas? SHOW YOUR WORK!
…Find all the possible ratios of molecules or atoms within a reaction…
5. What are the six possible ratios in the following reaction? (Notice that it is unbalanced and
must be balanced first.) Make sure to include “used” or “made” in each ratio.
H2O (l) + Na (s)
NaOH (aq) + H2 (g)
…write and balance chemical reactions from situations given…(for use later in stoichiometry problems)…
6. What is the balanced reaction for the production of mercury (II) nitrate and mercury from
mercury (II) oxide and nitrogen dioxide?
7. What is the balanced reaction for the combustion of butane (C4H10) to produce carbon dioxide
and water?
8. Write the balanced reaction for carbon dioxide and pure iron being produced from iron (III) oxide
and carbon.
…use balanced reactions to do simpler stoichiometry calculations
9. From reaction #10 above, how many moles of mercury (II) oxide would be needed to make 25
grams of mercury (II) nitrate?
10. From reaction #12 above, what mass of nitrogen dioxide would be needed to react completely
with 7.56 moles of mercury (II) oxide?
11. How much oxygen gas (moles) would produce 56.7 grams of carbon dioxide? (from rxn #11
above)
12. What mass of each product could be made from an excess of oxygen (as we have in our
atmosphere) and 1 kg of butane? See number 11 above.
17. The reaction in #12 above is used in industry to purify iron ore into iron. If 3 metric tons of iron
(III) oxide – called iron ore – were mined from the ground, how many grams of pure iron could
be produced from the reaction? (Hint: 1 metric ton = 1000 kg)
…Calculate percent yields from information given…
18. If you expect to produce 56 grams of something but get only 54 grams, what would your
percent yield be?
19. In reaction # 11 above, you burn 500 grams of butane in an excess of oxygen. What is your
percent yield if you collect 357.656 grams of water? (Hint: How much water should you have
collected?)
…Fact: if you hide my keys I will get you back and you will not like it…