| 1. Ten liters of a 0.1 M solution of MgCl2 would require how many moles of MgCl2 to prepare?
a. 1
b. 2
c. 3
d. 4
e. cannot be determined
2. Iron (III) oxide reacts with carbon to produce iron and one or more other products. Which of the following is most likely the other product(s)?
a. O2
b. C + O2
c. CO2
d. CH4
e. cannot be determined
3. In the reaction of iron (III) oxide with carbon, which of the following would be the most likely coefficient for the iron?
a. 1
b. 2
c. 3
d. 4
e. 5
4. In the reaction of iron (III) oxide with carbon, ten moles of iron(III) oxide would require how many moles of carbon to produce iron?
a. 10
b. 15
c. 20
d. 30
e. cannot be determined
5. In the reaction of iron (III) oxide with carbon, 159.6 g of iron(III)oxide would require how many grams of carbon to produce the maximum amount of iron?
a. 12 g
b. 18 g
c. 24 g
d. 36 g
e. cannot be determined
6. If 0.6 moles of sodium phosphate are reacted with 0.5 moles of iron (II) chloride, how many moles of iron (II) phosphate will be produced?
a. 0.1
b. 0.2
c. 0.3
d. 0.4
e. 0.6
7. If the molarity of the sodium phosphate is 0.2 M and the molarity of the iron(II) chloride is 0.3 M, what volumes of each would give the maximum amount of product?
a. 5 mL Na3PO4, 10 mL FeCl2
b. 10 mL Na3PO4, 5 mL FeCl2
c. 10 mL Na3PO4, 10 mL FeCl2
d. 15 mL Na3PO4, 5 mL FeCl2
e. 5 mL Na3PO4, 15 mL FeCl2
8. In the reaction: Zn + H2SO4 --> ZnSO4 + H2 which, if any, element is oxidized?
a. zinc
b. hydrogen
c. sulfur
d. oxygen
e. none is oxidized
9. How many mL of 0.250 M H2SO4 are required to react completely with 25.0 mL of 1.500 M NaOH?
a. 150. mL
b. 50.0 mL
c. 300. mL
d. 75.0 mL
e. none of these
10. What mass of iron(II) phosphate would be produced from mixing 200 ml of a 0.1 M solution of sodium phosphate and 300 mL of 0.1 M iron (II) chloride?
a. 3.57 g
b. 7.15 g
c. 10.72 g
d. 35.7 g
e. cannot be determined
11. The following reactions:Pb2+ + 2I- --> PbI2 2Ce4+ + 2I- --> I2 + 2Ce3+ HOAc + OH- --> H2O + OAc- are examples of which of the following?
a. acid-base reactions
b. oxidation reduction reactions
c. precipitation, acid-base, and redox reactions, respectively
d. redox, acid-base, and precipitation reactions, respectively
e. precipitation, redox, and acid-base reactions, respectively
12. In writing the total ionic equation for the reaction (if any) that occurs when solutions of KOH and Mg(NO3)2 are mixed, which of the following would NOT be written as ionic species?
a. KOH
b. Mg(NO3) 2
c. Mg(OH)2
d. KNO3
e. All of the above would be written as ionic species
13. Given the problem, Determine the number of grams of iron required to completely replace copper in 250 mL of a 0.10 M solution of CuSO4, which of the following would be a most likely first step in the solution?
a. Convert molarity to moles.
b. Find the molar mass of copper sulfate
c. Write a balanced equation for the replacement reaction.
d. Determine the number of grams of copper sulfate in solution.
e. None of the above
14. How many moles of silver sulfide are formed when 269.7 grams of silver metal react with excess sulfur?
a. 154.84 g
b. 309.67 g
c. 464.51 g
d. 516.38 g
e. none of the above
15. How many grams of solute are in 250.0 mL of 4.00 M CaCl2?
a. 55.5 g
b. 5.55 g
c. 11.1 g
d. 111.1 g
e. none of the above
16. When 6.57 g of iron were reacted with excess hydrochloric acid (HCl), hydrogen gas and 14.63 grams of iron (II) chloride were produced. Which of the following is the theoretical yield of iron (II) chloride?
a. 15.00 grams
b. 14.96 grams
c. 14.63 grams
d. 14.25 grams
e. none of the above
17. For the reaction in the above problem, what is the percent yield or iron (II) chloride in the reaction?
a. 97.99%
b. 98.58%
c. 99.21
d. 102.1%
e. none of the above
18. How many grams of oxygen gas are required to react completely with 14.6 grams of solid sodium metal to form sodium oxide?
a. 5.08 grams
b. 2.54 grams
c. 10.2 grams
d. 6.84 grams
e. none of the above
19. How many grams of copper will be required to completely replace silver from 208 mL of a 0.100 M solution of silver nitrate (AgNO3) if the product solution is copper (II) nitrate?
a. 6.60 grams
b. 3.30 grams
c. 2.64 grams
d. 0.66 grams
e. none of the above
20. When a solution of zinc bromide is mixed with a solution of calcium hydroxide a white precipitate of zinc hydroxide is formed. If 250 mL of 0.5 M zinc bromide is mixed with 75 mL of 0.75 M calcium hydroxide, what is the expected mass of zinc hydroxide that will be produced?
a. 1.45 g
b. 8.96 g
c. 12.43 g
d. 5.59 g
e. none of the above
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