2nd Semester Chemistry-575 Final Exam Review Answer Section
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1 2nd Semester Chemistry-575 Final Exam Review Answer Section MULTIPLE CHOICE 1. ANS: B PTS: 1 DIF: L2 REF: p. 290 p. 291 OBJ: Relate Avogadro s number to a mole of a substance. 2. ANS: B Mole ratio is 2 moles Al for 3 moles FeO. Therefore 1 mole Al would only need 1.5 moles of FeO. No need for mole island if you have nice whole numbers. PTS: 1 DIF: L1 REF: p. 359 p. 360 OBJ: Construct mole ratios from balanced chemical equations and apply these ratios in mole-mole stoichiometric calculations. STA: 12.C.5.a 3. ANS: B -Emperical formulas are like a reduced formula in math; the lowest ratio of the elements. -The molecular formula is the actual number of atoms of each element in the molecule. -The molar mass should match the molecular formula. -90 g/mole is the mass of C3H12N3. C3H12N3 can be reduced to CH4N by dividing by 3. PTS: 1 DIF: L2 REF: p. 312 OBJ: Distinguish between empirical and molecular formulas. 4. ANS: A PTS: 1 DIF: L1 REF: p. 424 OBJ: Use the combined gas law to solve problems. 5. ANS: C P1V1/T1 = P2V2/T2 Don t forget to convert temperatures to Kelvins PTS: 1 DIF: L2 REF: p. 419 OBJ: Use the combined gas law to solve problems. 6. ANS: C PTS: 1 DIF: L1 REF: p. 426 OBJ: Compute the value of an unknown variable in the equation for the ideal gas law. 7. ANS: D PV=nRT Don t forget to convert temperatures to Kelvins PTS: 1 8. ANS: A PTS: 1 DIF: Medium OBJ: 2.3A TOP: Charles's Law SEC: A 1
2 9. ANS: A Section : A PTS: 1 DIF: Medium OBJ: 2.4A TOP: Temperature and Pressure SEC: A 10. ANS: B PTS: 1 DIF: L1 REF: p. 386 OBJ: Interpret gas pressure in terms of kinetic theory. 11. ANS: B -High pressure pushes down on the surface of mercury in a thermometer making the mecury rise. -Low pressure does not push on the surface of mercury in a thermometer so the level of mecury falls. PTS: 1 DIF: L1 REF: p. 386 OBJ: Interpret gas pressure in terms of kinetic theory. 12. ANS: A PTS: 1 DIF: Medium OBJ: 4.4B TOP: Solubility Curves 13. ANS: C -Normally if you try to go above the solubility curve, the solution would be saturated and there would be undissolved solute on the bottom. -In this question, they stipulate that all 80 grams dissolved. This would be a rare example of a solution that had become supersaturated. -Supersatruated means that more is dissolved than should actually be dissolved at a given temperature. PTS: 1 DIF: Medium OBJ: 4.4B TOP: Solubility Curves 14. ANS: A polar dissolves polar non-polar dissolves non-polar ionic solids are very polar so will dissolve in polar substances like water PTS: 1 DIF: Medium OBJ: 4.1B TOP: Polarity 15. ANS: D PTS: 1 DIF: L1 REF: p. 481 OBJ: Solve problems involving the molarity of a solution. 2
3 16. ANS: B You need to convert the grams of solute to moles. Convert the volume of liquid from ml to Liters. PTS: 1 DIF: L3 REF: p. 481 OBJ: Solve problems involving the molarity of a solution. 17. ANS: A PTS: ANS: D PTS: ANS: A PTS: 1 DIF: L1 REF: p. 508 OBJ: Identify the units used to measure heat transfer. 20. ANS: C q=mc t rearrange the formula to solve for t t = q/mc solve for the change in temperature. Substances with low specific heats like lead heat up quickly. Substances with high specific heats like water need a lot of energy to increase their temperature. PTS: 1 DIF: L1 REF: p. 509 p. 510 OBJ: Identify the units used to measure heat transfer. 21. ANS: A Energy always moves into or out of a system during phase changes. Solids have the least energy, gasses have the most energy. If you want to move from a solid to liquid, and from a liquid to gas, you would need to add energy. The opposite is also true. When you move from a gas to a liquid, and from a liquid to a solid, substances release energy to their surroundings. PTS: 1 DIF: L2 REF: p. 512 OBJ: Describe how calorimeters are used to measure heat flow. 22. ANS: A Endothermic reactions must absorb energy so energy must be on the reactant side. Exothermic reactions would have energy on thr product side. 3
4 23. ANS: A Phase changes occur during the flat spots. 24. ANS: B A-B = solid B-C = solid and liquid C-D = liquid D-E = liquid and gas E-F = gas 25. ANS: B A-B = KE changing B-C = PE changing C-D =KE changing D-E = PE changing E-F = KE changing 26. ANS: A Endothermic reactions absorb energy. The products have more energy than the reactants. Remember this is an energy graph, not a temperature graph. 27. ANS: B Endothermic reactions gain energy so the change in potential energy would be positive. Exothermic reactions drop in PE so would be reported as negative. 28. ANS: B The energy needed to get over the hump is the activation energy. 29. ANS: B PTS: 1 4
5 30. ANS: B ph + poh = 14. When the OH - ions increase, the H + ions decrease. When H+ ions increase, OH - ions decrease. Acids have a higher H + Bases have a lower H + Acids 0-7 Bases 7-14 Neutral 7 PTS: 1 5
2nd Semester Chemistry-575 Final Exam Review
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