CHE201-174 L Chapters 3-4 Practice TEST PDF

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professor walker, chapter 3 and 4 practice test with answers attached ...

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CHE 201-174 L CHAPTERS 3-4 PRACTICE TESTS

3/26/20

READ ALL DIRECTIONS CAREFULLY BEFORE ANSWERING ANY ITEM BELOW. Multiple Choice Identify the choice that best completes the statement or answers the question.

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1. Consider the element indium, atomic number 49, atomic mass 114.8 g. The nucleus of an atom of indium-112 contains A) 49 protons, 63 neutrons, 49 electrons B) 49 protons, 49 neutrons C) 49 protons, 49 alpha particles D) 49 protons, 63 neutrons E) 49 protons, 112 neutrons

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2. Naturally occurring copper exists in two isotopic forms: 63Cu and 65Cu. The atomic mass of copper is 63.55 amu. What is the approximate natural abundance of 63Cu? A) 63% B) 90% C) 70% D) 50% E) 30%

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3. Naturally occurring element X exists in three isotopic forms: X-28 (27.977 amu, 92.23% abundance), X-29 (28.976 amu, 4.67% abundance), and X-30 (29.974 amu, 3.10% abundance). Calculate the atomic weight of X. A) 28.09 amu B) 48.63 amu C) 27.16 amu D) 28.97 amu E) 86.93 amu

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4. How many moles of hydrogen sulfide are contained in a 49.7-g sample of this gas? A) 0.686 mol B) 1.46 mol C) 83.8 mol D) 24.7 mol E) 2.92 mol

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5. For which compound does 0.256 mole weigh 12.8 g? A) C2H4O B) CO2 C) CH3Cl D) C2H6 E) none of these

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6. Calculate the molar mass of barium sulfite. A) 233.40 g/mol B) 201.40 g/mol

C) 354.73 g/mol D) 514.87 g/mol E) 217.40 g/mol ____

7. Which compound contains the highest percent by mass of hydrogen? A) HCl B) H2O C) H2SO4 D) H2S E) HF

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8. A compound composed of sulfur and fluorine is found to contain 62.79% by mass of sulfur. If the molar mass of the compound is 102.13 g/mol, what is its molecular formula? A) S3F B) S2F4 C) SF D) S2F E) S2F2

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9. How many of the following are true concerning balanced chemical equations? I. The number of molecules is conserved. II. The coefficients for the reactants tell you how much of each reactant you are given. III. Atoms are neither created nor destroyed. IV. The coefficients indicate the mass ratios of the substances used. V. The sum of the coefficients on the reactant side equals the sum of the coefficients on the product side. A) B) C) D) E)

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1 2 3 4 5

10. Which of the following equations is not balanced? A) 4Al + 3O2 → 2Al2O3 B) C2H6 + O2 → 2CO2 + 3H2O C) 2KClO3 → 2KCl + O2 D) 4P4 + 5S8 → 4P4S10 E) P4 + 5O2 → P4O10

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11. What is the sum of the coefficients of the following equation when it is balanced using smallest whole numbers? NaNH2 + NaNO3 → NaN3 +NaOH + NH3 A) 5 B) 6 C) 7 D) 8

E) 9 ____

12. A 7.11-g sample of potassium chlorate was decomposed according to the following equation: 2KClO3 → 2KCl + 3O2 How many moles of oxygen are formed? A) 2.78 g B) 0.0580 mol C) 0.0387 mol D) 0.0870 mol E) none of these

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13. Phosphorus, P4, can be prepared from calcium phosphate by the reaction 3370 g 1795 g 650 g 2Ca3(PO4)2 + 310 g/mol

6SiO2 60.1 g/mol

+

10C

→ 6CaSiO3 + P4 + 10CO

12.0 g/mol

The molar mass for each reactant is shown below the reactant, and the mass of each reactant for this problem is given above. Which reactant is the limiting reagent? A) C B) SiO2 C) Ca3(PO4)2 D) P4 E) More information is needed. ____

14. The reaction of 11.9 g of CHCl3 with excess chlorine produced 10.2 g of CCl4, carbon tetrachloride: What is the percent yield? A) 100% B) 33.2% C) 66.3% D) 86% E) 44.2%

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15. The interaction between solute particles and water molecules, which tends to cause a salt to fall apart in water, is called A) hydration B) polarization C) dispersion D) coagulation E) conductivity

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16. Which of the following is paired incorrectly? A) H2SO4 – strong acid B) HNO3 – weak acid C) Ba(OH)2 – strong base

D) HCl – strong acid E) NH3 – weak base ____

17. The man who discovered the essential nature of acids through solution conductivity studies is A) Priestly B) Boyle C) Einstein D) Mendeleev E) Arrhenius

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18. A 16.4-g sample of HF is dissolved in water to give 2.0  102 mL of solution. The concentration of the solution is: A) 0.82 M B) 0.16 M C) 0.08 M D) 4.1 M E) 8.2 M

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19. Which of the following aqueous solutions contains the greatest number of ions? A) 400.0 mL of 0.10 M NaCl B) 300.0 mL of 0.10 M CaCl2 C) 200.0 mL of 0.10 M FeCl3 D) 200.0 mL of 0.10 M KBr E) 800.0 mL of 0.10 M sucrose

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20. A 38.1-g sample of SrCl2 is dissolved in 112.5 mL of solution. Calculate the molarity of this solution. A) 27.0 M B) 2.14 M C) 53.7 M D) 0.339 M E) none of these

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21. A 74.28-g sample of Ba(OH)2 is dissolved in enough water to make 2.450 liters of solution. How many mL of this solution must be diluted with water in order to make 1.000 L of 0.100 M Ba(OH)2? A) 565 mL B) 177 mL C) 17.7 mL D) 4.34 mL E) 231 mL

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22. The following reactions 2K(s) + Br2(l) → 2KBr(s) AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) HCl(aq) + KOH(aq) → H2O(l) + KCl(aq) are examples of A) precipitation reactions

B) C) D) E)

redox, precipitation, and acid-base, respectively precipitation (two) and acid-base reactions, respectively redox reactions none of these

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23. Aqueous solutions of sodium sulfide and copper(II) chloride are mixed together. Which statement is correct? A) Both NaCl and CuS precipitate from solution. B) No reaction will occur. C) CuS will precipitate from solution. D) NaCl will precipitate from solution. E) A gas is released.

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24. Which of the following salts is insoluble in water? A) Na2S B) K2CO3 C) Pb(NO3)2 D) CaCl2 E) All of these are soluble in water.

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25. In the balanced molecular equation for the neutralization of sodium hydroxide with sulfuric acid, the products are: A) NaSO4 + H2O B) NaSO3 + 2H2O C) 2NaSO4 + H2O D) Na2S + 2H2O E) Na2SO4 + 2H2O

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26. Sulfamic acid, HSO3NH2 (molar mass = 97.1 g/mol), is a strong monoprotic acid that can be used to standardize a strong base:

A 0.165-g sample of HSO3NH2 required 19.4 mL of an aqueous solution of KOH for a complete reaction. What is the molarity of the KOH solution? A) 0.00170 M B) 8.76 M C) 0.0876 M D) 0.0330 M E) none of these ____

27. The oxidation state of iodine in IO3– is: A) 0 B) +3 C) –3 D) +5 E) –5

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28. Which of the following statements is not true?

A) When a metal reacts with a nonmetal, an ionic compound is formed. B) A metal-nonmetal reaction can always be assumed to be an oxidation-reduction reaction. C) Two nonmetals can undergo an oxidation-reduction reaction. D) When two nonmetals react, the compound formed is ionic. E) A metal-nonmetal reaction involves electron transfer. ____

29. In the reaction 2Cs(s) + Cl2(g) → 2CsCl(s), Cl2 is A) the reducing agent B) the oxidizing agent C) oxidized D) the electron donor E) two of these

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30. Which of the following statements is(are) true? Oxidation and reduction A) cannot occur independently of each other B) accompany all chemical changes C) describe the loss and gain of electron(s), respectively D) result in a change in the oxidation states of the species involved E) A, C, and D

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31. Balance the following oxidation-reduction reaction using the oxidation number method: Fe + Br2 → Fe3+ + Br– In the balanced equation, the coefficient of Br– is A) 2 B) 3 C) 4 D) 6 E) none of these

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32. The MnO4– is often used to analyze for the Fe2+ content of an aqueous solution via the reaction MnO4–(aq) + Fe2+(aq) + H+(aq) → Fe3+(aq) + Mn2+(aq) + H2O(l) What is the ratio of Fe2+ : MnO4– in the balanced equation? A) 1 : 1 B) 2 : 1 C) 3 : 1 D) 4 : 1 E) 5 : 1

Short Answer

1. In order to determine the molecular formula from the empirical formula, we must know the __________. 2. In a chemical equation, the _________ are written on the left side of the arrow, and the _________ are written on the right side of the arrow.

3. The __________ in a balanced equation represent numbers of molecules. 4. A molecule with an unequal charge distribution is said to be a __________ molecule. 5. Soluble ionic compounds containing the hydroxide ion are called strong __________. 6. A __________ is a substance dissolved in a liquid to make a solution. 7. A __________ electrolyte dissociates to a great extent in an aqueous solution. 8. Molarity is defined as __________ of solute per volume of solution in ___________.

CHE 201-174 L CHAPTERS 3-4 PRACTICE TESTS Answer Section

3/26/20

MULTIPLE CHOICE 1. ANS: D PTS: 1 DIF: Easy REF: 3.2 KEY: Chemistry | general chemistry | early atomic theory | atomic theory of matter | structure of the atom MSC: Conceptual 2. ANS: C PTS: 1 DIF: Moderate REF: 3.2 KEY: Chemistry | general chemistry | early atomic theory | atomic theory of matter | atomic weight | mass spectroscopy MSC: Quantitative 3. ANS: A PTS: 1 DIF: Easy REF: 3.2 KEY: Chemistry | general chemistry | early atomic theory | atomic theory of matter | atomic weight | mass spectroscopy MSC: Quantitative 4. ANS: B PTS: 1 DIF: Easy REF: 3.4 KEY: Chemistry | general chemistry | stoichiometry | mass and moles of substance | mole MSC: Quantitative 5. ANS: C PTS: 1 DIF: Easy REF: 3.4 KEY: Chemistry | general chemistry | stoichiometry | mass and moles of substance | mole MSC: Quantitative 6. ANS: E PTS: 1 DIF: Moderate REF: 3.4 KEY: Chemistry | general chemistry | stoichiometry | mass and moles of substance | molecular weight MSC: Conceptual 7. ANS: B PTS: 1 DIF: Easy REF: 3.6 KEY: Chemistry | general chemistry | stoichiometry | determining chemical formulas | mass percentage MSC: Quantitative 8. ANS: E PTS: 1 DIF: Easy REF: 3.7 KEY: Chemistry | general chemistry | stoichiometry | determining chemical formulas | molecular formula MSC: Quantitative 9. ANS: A PTS: 1 DIF: Easy REF: 3.8 KEY: Chemistry | general chemistry | early atomic theory | chemical equation | balancing chemical equation MSC: Conceptual 10. ANS: C PTS: 1 DIF: Easy REF: 3.9 KEY: Chemistry | general chemistry | early atomic theory | chemical equation | balancing chemical equation MSC: Conceptual 11. ANS: E PTS: 1 DIF: Easy REF: 3.9 KEY: Chemistry | general chemistry | early atomic theory | chemical equation | balancing chemical equation MSC: Conceptual 12. ANS: D PTS: 1 DIF: Easy REF: 3.1 KEY: Chemistry | general chemistry | stoichiometry | stoichiometry calculation | amounts of substances MSC: Quantitative 13. ANS: B PTS: 1 DIF: Moderate REF: 3.11 KEY: Chemistry | general chemistry | stoichiometry | stoichiometry calculation | limiting reactant MSC: Conceptual

14. ANS: C PTS: 1 DIF: Moderate REF: 3.11 KEY: Chemistry | general chemistry | stoichiometry | stoichiometry calculation | limiting reactant MSC: Quantitative 15. ANS: A PTS: 1 DIF: Easy REF: 4.1 KEY: Chemistry | general chemistry | solutions | solution formation MSC: Conceptual 16. ANS: B PTS: 1 DIF: Easy REF: 4.2 KEY: Chemistry | general chemistry | chemical reactions | ions in aqueous solution | electrolyte MSC: Conceptual 17. ANS: E PTS: 1 DIF: Easy REF: 4.2 KEY: Chemistry | general chemistry | chemical reactions | ions in aqueous solution | electrolyte MSC: Conceptual 18. ANS: D PTS: 1 DIF: Easy REF: 4.3 KEY: Chemistry | general chemistry | chemical reactions | working with solutions | concentration MSC: Quantitative 19. ANS: B PTS: 1 DIF: Easy REF: 4.3 KEY: Chemistry | general chemistry | chemical reactions | working with solutions | concentration MSC: Conceptual 20. ANS: B PTS: 1 DIF: Easy REF: 4.3 KEY: Chemistry | general chemistry | chemical reactions | working with solutions | concentration MSC: Quantitative 21. ANS: A PTS: 1 DIF: Moderate REF: 4.3 KEY: Chemistry | general chemistry | chemical reactions | working with solutions | diluting solutions MSC: Quantitative 22. ANS: B PTS: 1 DIF: Easy REF: 4.4 KEY: Chemistry | general chemistry | chemical reactions | types of chemical reactions MSC: Conceptual 23. ANS: C PTS: 1 DIF: Easy REF: 4.5 KEY: Chemistry | general chemistry | chemical reactions | ions in aqueous solution | solubility rules MSC: Conceptual 24. ANS: E PTS: 1 DIF: Easy REF: 4.5 KEY: Chemistry | general chemistry | chemical reactions | ions in aqueous solution | solubility rules MSC: Conceptual 25. ANS: E PTS: 1 DIF: Easy REF: 4.8 KEY: Chemistry | general chemistry | chemical reactions | types of chemical reactions | acid-base reaction | neutralization reaction MSC: Conceptual 26. ANS: C PTS: 1 DIF: Easy REF: 4.8 KEY: Chemistry | general chemistry | chemical reactions | quantitative analysis | volumetric analysis MSC: Quantitative 27. ANS: D PTS: 1 DIF: Easy REF: 4.9 KEY: Chemistry | general chemistry | chemical reactions | types of chemical reactions | oxidation-reduction reaction | assigning oxidation number MSC: Conceptual 28. ANS: D PTS: 1 DIF: Easy REF: 4.9 KEY: Chemistry | general chemistry | chemical reactions | types of chemical reactions | oxidation-reduction reaction MSC: Conceptual

29. ANS: B PTS: 1 DIF: Easy REF: 4.9 KEY: Chemistry | general chemistry | chemical reactions | types of chemical reactions | oxidation-reduction reaction MSC: Conceptual 30. ANS: E PTS: 1 DIF: Easy REF: 4.9 KEY: Chemistry | general chemistry | chemical reactions | types of chemical reactions | oxidation-reduction reaction MSC: Conceptual 31. ANS: D PTS: 1 DIF: Easy REF: 4.1 KEY: Chemistry | general chemistry | chemical reactions | types of chemical reactions | balancing oxidation-reduction equations | oxidation number method MSC: Conceptual 32. ANS: E PTS: 1 DIF: Moderate REF: 4.1 KEY: Chemistry | general chemistry | chemical reactions | types of chemical reactions | balancing oxidation-reduction equations | oxidation number method MSC: Conceptual SHORT ANSWER 1. ANS: molar mass PTS: 1 DIF: Easy REF: 3.7 KEY: Chemistry | general chemistry | stoichiometry | determining chemical formulas | molecular formula MSC: Conceptual 2. ANS: reactants, products PTS: 1 DIF: Easy REF: 3.8 KEY: Chemistry | general chemistry | early atomic theory | chemical equation | writing equation MSC: Conceptual 3. ANS: coefficients PTS: 1 DIF: Easy REF: 3.8 KEY: Chemistry | general chemistry | early atomic theory | chemical equation | writing equation MSC: Conceptual 4. ANS: polar PTS: 1 DIF: Easy REF: 4.1 KEY: Chemistry | general chemistry | solutions | solution formation MSC: Conceptual 5. ANS: bases PTS: 1 DIF: Easy REF: 4.2 KEY: Chemistry | general chemistry | chemical reactions | types of chemical reactions | acid-base reaction | base definition MSC: Conceptual

6. ANS: solute PTS: 1 DIF: Easy REF: 4.2 KEY: Chemistry | general chemistry | solutions | solution formation | types of solutions MSC: Conceptual 7. ANS: strong PTS: 1 DIF: Easy REF: 4.2 KEY: Chemistry | general chemistry | chemical reactions | ions in aqueous solution | electrolyte | strong electrolyte MSC: Conceptual 8. ANS: moles, liters PTS: 1 DIF: Easy REF: 4.3 KEY: Chemistry | general chemistry | chemical reactions | working with solutions | concentration MSC: Conceptual...