Quarter 3 Exam Review

1. Quarter 3 Exam Review

2. Which of the following describes intermolecular forces? A. Intermolecular forces are forces found in ionic compounds.   • B. Intermolecular forces are repulsive forces that exist between molecules   • C. Intermolecular forces are covalent bonds within a molecule   • D. Intermolecular forces are attractive forces that exist between molecules

3. Which of the following is not a property of liquids? A. Liquids have definite volume  B. Liquids have high densities in comparison to gases   C. Liquids flow  D.  Liquids have definite shape

4. Which of the following has dipole-dipole forces? A. CO2 B.  CH2F2 C. CCl4 D. Ne

5. Which of the following has hydrogen bonding? • HF   • HCl • HBr • H2

6. What is the molarity of a solution that contains 122 g of MgSO4 in 3.50 L of solution? A. 0.550 MB. 0.281 MC. 0.290 MD. 0.630 M

7. How many moles of KI are present in 0.85 L of a 0.55 M KI solution? A. 3.1 molsB. 1.6 molsC. 0.94 molsD. 0.47 mols

8. What is the molality of a solution that contains 68.0 g of NaOH in 500. g of solution? A. 1.70 mB. 0.0034 mC. 1.18 mD. 3.40 m

9. You are given 100.0 ml of a 2 M solution of KOH. What would be the molarity of the solution if it is diluted to a volume of 1000 ml? A. 0.2 MB. 0.002 MC. 2 MD. 0.02 M

10. You have 200.0 ml of a 7.17 M KNO3. What would be the new volume if you diluted the solution to a molarity of 0.35 M? A. 45.1 LB. 4.10 LC. 2.51 LD. 26.05 L

11. At constant temperature, a change in volume will NOT affect the equilibrium of substances present in which of the following?

12. An equal number of moles of each of the reactants are sealed in a container and allowed to come to the equilibrium. At equilibrium which of the following must be true? I [CO2] must equal [H2O] II [O2] must be less than [C2H4] III [CO2] must be greater than [C2H4] A. II and III B. I only C. III only D. II only E. I and II

13. Which of the following gases will have the fastest rate of effusion? • H2 • He •  N2 • Ne   • CO

14. A gas mixture contains 2.0 moles of helium and 8.0 moles of carbon dioxide and is held under conditions of standard temperature and pressure. What is the partial pressure of the carbon dioxide? • 2.0atm    • 0.2atm    • 8.0atm   • 0.8 atm • none of these

15. A gas that is confined in a rigid container is heated. Which of the following statements is true? • a)       the kinetic energy of the gas particles will decrease • b)       the pressure will increase • c)       the density will decrease • d)       the number of moles of gas will increase • e)       the volume will increase

16. Which gas deviates MOST from ideal behavior? • a) SO2 •  b) Ne    • c) CH4 • d) N2 •  e) H2

17. An 11.2L container will hold about 8.5g of which of the following gases at 0˚C and 1atm? • a) SO2 • b) N2 • c) CO2 • d) C4H8 • e) NH3

18. Colligative properties depend on which of the following? • A. The polarity of the solutes. • B. The number of ions the solute dissociate into. • C. The freezing point of the solute. • D. The solubility of the solvent.

19. Which of the following statements are true? • A. Temperature changes after a liquid melted but before it starts to boil. • B. Heat changes while a solution is boiling. • C. A substances boiling point is always the same temperature. • D. The freezing point of substance is dependant on the amount of liquid.

20. A solution is prepared by dissolving 22.5 g of RbBr in 250 g of water. Calculate its theoretical freezing point. • A. -1.01 °C • B. -.277 °C • C. -2.02 °C • D. -.544°C

21. Most sulfate salts are soluble. Important exceptions to this rule include BaSO4, PbSO4, Ag2SO4 and SrSO4 .  Salts containing nitrate ion (NO3-) are generally soluble. • When solutions of lead (II) nitrate and iron(III) sulfate are mixed, what is the net ionic reaction? • A. Fe+3(aq) + 3 NO3-(aq) Fe(NO3)3(s) • B. Pb+2(aq) + SO4(aq) PbSO4(s) • C. 2 Fe+3(aq) + 3 SO4(aq) Fe2(SO4)3(s) • D. Pb+2(aq) + 2 NO3-(aq)Pb(NO3-)(s)

22. What is the concentration of nitrate ions in a 0.225M solution of iron(III) nitrate • A. 0.225 M • B. 0.450 M • C. 0.675 M • D. 0.900 M

23. In a reaction, 12.5 mL of 0.120M Pb(NO3)2 is mixed with 15.0 mL of 0.180 M NaCl solution. What mass of lead(II) chloride will be produced? • A. 0.750 g • B. 0.00135 g • C. 0.375 g • D. 0.00270 g

24. Salts containing Cl-, Br -, I - are generally soluble. Important exceptions to this rule are halide salts of Ag+, Pb2+, and (Hg2)2+. Thus, AgCl, PbBr2, and Hg2Cl2are all insoluble. • In a reaction, 12.5 mL of 0.120M Pb(NO3)2 is mixed with 15.0 mL of 0.180 M NaCl solution. What is the concentration of Cl ion after the reaction? • A. 0 M • B. .0982M • C. .360M • D. none of the above

25. In a reaction, 12.5 mL of 0.120M Pb(NO3)2 is mixed with 15 mL of 0.180 M NaCl solution. What is the concentration of NO3 ion ion after the reaction? • A. 0 M • B. .240M • C. .109M • D. none of the above 0.00300 M ?

26. Question 3 • What is the density (g/L) of helium gas inside a container that reads an internal pressure and temperature of 18.5atm and 20.0˚C respectively? • 45.0 g/L • 3.08 g/L • 0.325 g/L • I dunno, but if you breathed some of it in you sure would sound funny!

27. Question 4 • Which of the following atoms are notorious for forming network covalent bonds when bonded to themselves or to each other? • Carbon • Tungsten • Silicon • All of these

28. Question 5 • The intermolecular attraction in the list below is • Polar Covalent Bond • Ionic Bond • Hydrogen Bond • Nonpolar Covalent Bond

29. The graph shows the variation of concentration with time for the reaction at 25 °C: • 3A(aq) <--> B(aq) + 2C(aq) • What is the value of the equilibrium constant at time t2? • (A)1.189 (B)0.845(C)0.567(D)0.222

30. Consider this diagram: