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1 Final Prep Chap 8&9 (DO NOT WRITE ON THIS TEST) Multiple Choice Identify the choice that best completes the statement or answers the question. 1. After the correct formula for a reactant in an equation has been written, the a. subscripts are adjusted to balance the equation. b. formula should not be changed. c. same formula must appear as the product. d. symbols in the formula must not appear on the product side of the equation. 2. A chemical formula written over the arrow in a chemical equation signifies a. a byproduct. c. a catalyst for the reaction. b. the formation of a gas. d. an impurity. 3. Which coefficients correctly balance the formula equation CaO + H 2 O Ca(OH) 2? a. 2, 1, 2 c. 1, 2, 1 b. 1, 2, 3 d. 1, 1, 1 4. In what kind of reaction does a single compound produce two or more simpler substances? a. decomposition reaction c. single-replacement reaction b. synthesis reaction d. ionic reaction 5. The equation A + BX AX + B is the general equation for a a. double-replacement reaction. c. single-replacement reaction. b. decomposition reaction. d. combustion reaction. 6. In what kind of reaction do the ions of two compounds exchange places in aqueous solution to form two new compounds? a. synthesis reaction c. decomposition reaction b. double-replacement reaction d. combustion reaction 7. The reaction 2Mg(s) + O 2 (g) 2MgO(s) is a a. synthesis reaction. c. single-replacement reaction. b. decomposition reaction. d. double-replacement reaction. 8. In one type of synthesis reaction, an element combines with oxygen to yield a(n) a. acid. c. oxide. b. hydroxide. d. metal. 9. When heated, a metal carbonate decomposes into a metal oxide and a. carbon. c. oxygen. b. carbon dioxide. d. hydrogen. 10. The formulas for the products of the reaction between sodium hydroxide and sulfuric acid are a. Na 2 SO 4 and H 2 O. c. SI 4 and Na 2 O. b. NaSO 4 and H 2 O. d. S + O 2 and Na. 11. Predict what happens when nickel is added to a solution of potassium chloride. a. No reaction occurs. c. Potassium nickel chloride forms. b. Nickel chloride forms. d. Hydrochloric acid forms.
2 12. Which reaction can be predicted from the activity series? a. 2Cl Cl2 c. 2HCl + 2Na 2NaCl + H b. HCl + NaOH NaCl + H 2 O d. Cl 2 2Cl 13. In the chemical reaction wa + xb yc + zd, a comparison of the number of moles of A to the number of moles of C would be a(n) a. mass ratio. c. electron ratio. b. mole ratio. d. energy proportion. 14. For the reaction N 2 + 3H 2 2NH 3, how many moles of nitrogen are required to produce 18 mol of ammonia? a. 9.0 mol c. 27 mol b. 18 mol d. 36 mol Element Symbol Atomic mass Bromine Br Calcium Ca Carbon C Chlorine Cl Cobalt Co Copper Cu Fluorine F Hydrogen H Iodine I Iron Fe Lead Pb Magnesium Mg Mercury Hg Nitrogen N Oxygen O Potassium K Sodium Na Sulfur S For the reaction 3Fe + 4H 2 O Fe 3 O 4 + 4H 2, how many moles of iron oxide are produced from 500 g of iron? a. 1 mol c. 9 mol b. 3 mol d. 12 mol 16. For the reaction SO 3 + H 2 O H 2 SO 4, how many grams of sulfuric acid can be produced from 200. g of sulfur trioxide and 100. g of water? a g c. 245 g b g d. 285 g 2
3 17. In the reaction A + B C + D, if the quantity of B is insufficient to react with all of A, a. A is the limiting reactant. c. there is no limiting reactant. b. B is the limiting reactant. d. no product can be formed. 18. What is the maximum possible amount of product obtained in a chemical reaction? a. theoretical yield c. mole ratio b. percent yield d. actual yield 19. A chemist interested in the efficiency of a chemical reaction would calculate the a. mole ratio. c. percent yield. b. energy released. d. rate of reaction. 20. A chemical reaction has NOT occurred if the products have a. the same mass as the reactants. b. less total bond energy than the reactants. c. more total bond energy than the reactants. d. the same chemical properties as the reactants. 21. To balance a chemical equation, it may be necessary to adjust the a. coefficients. c. formulas of the products. b. subscripts. d. number of products. 22. Which equation is NOT balanced? a. 2H 2 + O 2 2H 2 O b. 4H 2 + 2O 2 4H 2 O c. H 2 + H 2 + O 2 H 2 O + H 2 O d. 2H 2 + O 2 H 2 O 23. An active metal and a halogen react to form a(n) a. salt. c. acid. b. hydroxide. d. oxide. 24. In the equation 2Al(s) + 3Fe(NO 3 ) 2 (aq) 3Fe(s) + 2Al(NO 3 ) 3 (aq), iron has been replaced by a. nitrate. c. aluminum. b. water. d. nitrogen. 25. If a certain metal is placed in an ionic solution containing another metal and no reaction occurs, then the metal originally in the solution is a. a halogen. c. not on the activity series. b. higher on the activity series. d. unreactive. 26. A balanced chemical equation allows one to determine the a. mole ratio of any two substances in the reaction. b. energy released in the reaction. c. electron configuration of all elements in the reaction. d. mechanism involved in the reaction. 27. The coefficients in a chemical equation represent the a. masses, in grams, of all reactants and products. b. relative numbers of moles of reactants and products. c. number of atoms in each compound in a reaction. d. number of valence electrons involved in the reaction.
4 28. To determine the limiting reactant in a chemical reaction involving known masses of A and B, one could first calculate a. the mass of 100 mol of A and B. b. the masses of all products. c. the bond energies of A and B. d. the number of moles of B and the number of moles of A available. 29. What is the ratio of the actual yield to the theoretical yield, multiplied by 100%? a. mole ratio c. Avogadro yield b. percent yield d. excess yield Problem Element Symbol Atomic mass Bromine Br Calcium Ca Carbon C Chlorine Cl Cobalt Co Copper Cu Fluorine F Hydrogen H Iodine I Iron Fe Lead Pb Magnesium Mg Mercury Hg Nitrogen N Oxygen O Potassium K Sodium Na Sulfur S What mass in grams of hydrogen gas is produced if 20.0 mol of Zn are added to excess hydrochloric acid according to the equation Zn(s) +2HCl(aq) ZnCl 2 (aq) + H 2 ( )?
5 final Prep Answer Section MULTIPLE CHOICE 1. ANS: B PTS: 1 DIF: I OBJ: ANS: C PTS: 1 DIF: I OBJ: ANS: D PTS: 1 DIF: III OBJ: ANS: A PTS: 1 DIF: I OBJ: ANS: C PTS: 1 DIF: II OBJ: ANS: B PTS: 1 DIF: I OBJ: ANS: A PTS: 1 DIF: II OBJ: ANS: C PTS: 1 DIF: II OBJ: ANS: B PTS: 1 DIF: II OBJ: ANS: A PTS: 1 DIF: III OBJ: ANS: A PTS: 1 DIF: III OBJ: ANS: C PTS: 1 DIF: III OBJ: ANS: B PTS: 1 DIF: II OBJ: ANS: A PTS: 1 DIF: III OBJ: ANS: B PTS: 1 DIF: III OBJ: ANS: C PTS: 1 DIF: III OBJ: ANS: B PTS: 1 DIF: II OBJ: ANS: A PTS: 1 DIF: I OBJ: ANS: C PTS: 1 DIF: I OBJ: ANS: D PTS: 1 DIF: I OBJ: ANS: A PTS: 1 DIF: I OBJ: ANS: D PTS: 1 DIF: III OBJ: ANS: A PTS: 1 DIF: II OBJ: ANS: C PTS: 1 DIF: II OBJ: ANS: B PTS: 1 DIF: II OBJ: ANS: A PTS: 1 DIF: I OBJ: ANS: B PTS: 1 DIF: I OBJ: ANS: D PTS: 1 DIF: I OBJ: ANS: B PTS: 1 DIF: I OBJ: PROBLEM 30. ANS: 40.4 g H 2 PTS: 1 DIF: III OBJ: 9-3.2
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