How many grams of are produced when 3.00 g of burns according to this reaction? (Assume excess oxygen)
2. Ammonia burns in air according to the reaction shown below:

a) How many grams of NO form when react with 1.85 g of react with one another.
b) After the reaction above has completed, which reactant, and how much of it remains unreacted?
3. When 30.0 g of benzene and 65.0 g of bromine are reacted together as shown below, 56.7 g of bromobenzene ( ) is formed. What is the percent yield of this reaction?

acetylsalicylic acid
23.0 mL of 0.0770 M NaOH solution was used to completely react with the acid present in a aspirin tablet. What is the percent of acetylsalicylic acid in the aspirin tablet?
9. Concentrated nitric acid has a density of and contains by mass. What is the molarity of this solution?
10. How many grams of Na must react with 155 mL of water to produce a solution that is 0.175 M NaOH , as shown below. (Assume a final solution volume of 155 mL )

The mass of produced in this reaction was found to be 472 mg . Based on this information, what is the mass percent of calcium carbonate in limestone?
12. Identify each of the following substances as a non-electrolyte (NE), weak electrolyte (WE), or strong electrolyte (SE):
a)
b)
c)
d)
e) f)
13. Complete each equation shown below:
a)
b)
c)
14. Complete the molecular equations shown below, and write balanced net ionic equations for each:
a)
b)
15. For each reaction shown below, determine if a reaction occurs. If so, write a balanced net ionic equation. If not, write "No Rxn".
a)
b)
c)
d)
16. Write balanced net ionic equations for each reaction described below:
a) Solid sodium hydroxide pellets are dropped in solution of sulfuric acid.
b) Aqueous solutions of ammonium carbonate and calcium chloride are mixed together.
17. In the compounds below, assign oxidation numbers to the underlined element:
a)
b)
c)
d)
e)
g)
18. Identify which substance is oxidized and which substance is reduced, and determine the total number of electrons transferred in each of the following redox reactions.
a)
oxidized reduced # of
b)
oxidized reduced # of
c)
oxidized reduced # of
19. A solution is prepared by mixing 0.10 L of 0.12 M NaCl and 0.23 L of solutions. What volume of is required to precipitate all the chloride ions in the solution above? (Answer )
20. When reacts with water, it forms boric acid ( ) and hydrogen gas. Boric acid combines with sodium oxide to form borate salt and water. What mass of is required to form 151 g of the borate salt by this reaction sequence? (Answer )
21. Balance each oxidation or reduction half-reaction shown below:
a)
b)
c)
d)
22. What is the overall equation formed from combining half-reactions (b) and (d) above?
23. A person's blood alcohol can be determined by titrating a sample of blood plasma with a sodium dichromate solution. The balanced equation is:

If 35.46 mL of is required to titrate 25.00 g of plasma, what is the mass percent of alcohol in blood? (Answer )
24. Phosphoric acid can be produced by reaction of aqueous sodium phosphate and sulfuric acid. The other product in the reaction is sodium sulfate.
a) What volume (in mL ) of 1.55 M sulfuric acid is required to completely react with 27.5 mL of 1.20 M sodium phosphate?
b) What is the concentration of the phosphoric acid produced in the final solution?