3rd Nine weeks study guide
You need to know how to write formulas from names!!!!
Don’t forget to study your polyatomic ions again!!!
Complete the following on another sheet of paper.
How many moles of Pb is 9.3 x 1015 atoms of Pb?
What is the molar mass of ethane, C2H6?
Find the mass of 3.65 x102 mol K2SO4.
How many representative particles are in 2.5 mol H2O2?
What is the molar mass of each of the following compounds?
a. C6H12O6
b. NaHCO3 c. C7H12
d. KNH4SO4
6. Calculate the mass in grams of each of the following:
a. 8.0 mol lead oxide
d. 1.50 x 102 mol molecular oxygen
b. 0.75 mol hydrogen sulfide
e. 2.30 mol ethylene glycol (C2H6O2)
c. 0.00100 mol silicon tetrahydride
7. How many grams are in 1.73 mol of dinitrogen pentoxide?
8. How many grams are in 0.658 mol of calcium phosphate?
9. Calculate the number of moles in each of the following:
a. 0.50 g sodium bromide
d. 0.00100 g monochloromethane (CH3Cl)
b. 13.5 g magnesium nitrate
e. 1.50 x 103 g propylene glycol [C3H6(OH)2]
c. 1.02 g magnesium chloride
10. A chemist plans to use 435.0 grams of ammonium nitrate in a reaction. How many moles
of the compound is this?
11. A solution is to be prepared in a laboratory. The solution requires 0.0465 mol of quinine
(C20H24N2O2). What mass, in grams, should the laboratory technician obtain in order to
make the solution?
12. What is the volume at STP of 2.66 mol of methane (CH4) gas?
13. How many moles is 135 L of ammonia (NH3) gas at STP?
14. A sample of a compound analyzed in a chemistry laboratory consists of 5.34 g of carbon,
0.42 g of hydrogen, and 47.08 g of chlorine. What is the percent composition of this
compound?
15. Find the percent composition of a compound containing tin and chlorine if 18.35 g of the
compound contains 5.74 g of tin.
16. What is the mass of two moles of NaCl?
17. How many moles are in 16 grams of O2?
18. What is the volume of 16 grams of O2 at STP?
19. What is the percent composition of each of the following?
a. a. Cr2O3
c. HgS
b. b. Mn2P2O7
d. Ca(NO3)2
1.
2.
3.
4.
5.
20. Determine the empirical formula of the compound with the percent composition of 29.1%
Na, 40.5% S, and 30.4% O.
21. Determine the empirical formula of each of the following compounds from the
percent composition:
a. 7.8% carbon and 92.2% chlorine
b. 10.0% C, 0.80% H, 89.1% Cl
22. Calculate the percent by mass of water in Glauber’s salt (Na2SO4 • 10H2O).
23. What mass of sucrose, C12H22O11, is needed to make 300.0 mL of a 0.50M solution?
24. Calculate the molarity of each of the following solutions.
a. 0.40 mol of NaCl dissolved in 1.6 L of solution
b. 20.2 g of potassium nitratein enough water to make 250.0 mL of
solution
25. Calculate the number of grams of solute needed to prepare each of the
following solutions.
a. 2500.0 mL of a 3.0M solution of potassium hydroxide
b. 2.0 liters of 2.0M nitric acid solution
26. What is the molarity of a solution that contains 212.5 g of sodium nitrate in 3.0 liters of
solution?
27. Write the formulas for the following hydrates.
a. Calcium sulfate dihydrate
b. Cobalt(II) chloride hexahydrate
28. Write a balanced equation for each of these chemical reactions. Include appropriate
symbols for state.
a. Aluminum reacts with aqueous hydrochloric acid to form hydrogen gas and
aqueous aluminum chloride.
b. Acetylene gas (C2H2) burns in a welding torch with oxygen to form carbon
dioxide gas and water vapor.
29. Write the balanced equation for the reaction between hydrogen and oxygen that produces
water.
30. Write the balanced equation for the reaction that produces iron(II) sulfide from iron and
sulfur.
31. Write the balanced equation representing the heating of magnesium carbonate to produce
solid magnesium oxide and carbon dioxide gas.
32. Write a balanced equation for the production of HCl gas from its elements.
33. Write a balanced equation representing the formation of aqueous sulfuric acid from water
and sulfur trioxide gas.
34. Write a balanced equation from this word equation.
a. aqueous silver nitrate + copper metal  silver metal + aqueous copper nitrate
35. Write a balanced equation for the following word equation.
a. phosphorus + oxygen  tetraphosphorous decoxide
36. Write a balanced equation representing the reaction of magnesium with oxygen gas to
produce magnesium oxide.
37. Write the balanced equation for the reaction that occurs between aluminum and fluorine.
38. Write the balanced equation for the production of oxygen gas and potassium chloride
from the decomposition of potassium chlorate.
39. Write the balanced equation for the reaction between hydrochloric acid and calcium
metal. The products are hydrogen gas and calcium chloride.
40. Write the balanced equation for the combustion of propane (C3H8) to produce carbon
dioxide and water vapor.
41. Write the balanced equation for the reaction between iron(III) chloride and sodium
hydroxide. The products are iron(III) hydroxide and sodium chloride.
42. Classify each of the reactions in problems 38-43 as to type.
43. Use the activity series of metals (Table 11.2) and your knowledge of the relative
reactivity of the halogens to predict whether the following reactions will occur. Write
balanced equations for those reactions that do occur.
a. Br2(l) +NaCl(aq) 
b. Ca(s) + Mg(NO3)2(aq) 
c. K(s) + H2SO4(aq) 
d. Zn(s) + NaOH(aq) 
44. Identify the type of each of the following reactions.
a. 2C6H14(l ) + 19O2(g)  12CO2(g) + 14H2O(g)
b. 2Fe(s) + 3Br2(l )  2FeBr3(s)
45. Complete and balance the following equation. What must be true of one of the products
in order for a reaction to have taken place?
a. Li3PO4 + Zn(NO3)2
46. Identify the precipitate formed when solutions of the following ionic
compounds are mixed. If no precipitate is formed, write no precipitate.
a. Zn(NO3)2 + SnCl2 
b. KCl + AgNO3 
c. Cu(NO3)2 + Na2S 
d. Al2(SO4)3 + 3Mg(OH)2 
e. AgNO3(aq) + NaCl(aq) 
f. CaCl2(aq) + Na2CO3(aq) 
g. Fe(NO3)3(aq) + KCl(aq) 
h. Pb(NO3)2(aq) + HCl(aq) 