Chemistry 1120 Final Exam Study Guide
Chemistry 1120 Final Exam Study Guide Chem 1120-001
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This 7 page Study Guide was uploaded by Callie Simpson on Sunday April 24, 2016. The Study Guide belongs to Chem 1120-001 at East Carolina University taught by James E. Collins in Winter 2016. Since its upload, it has received 50 views. For similar materials see Introduction to Chemistry for the Allied Health Sciences in Science at East Carolina University.
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Date Created: 04/24/16
Name: Chemistry 1120 Final Exam Study Guide Some Useful Quantities: N = 6.02 x 10 (Avogadro's Number) R = 0.0821 L•atm/mol•K 1. Which of the following molecules in the pure liquid state would be expected to hydrogen bond? H H H C N C H H H H H H C O H H C H H C F H H H (1) (2) (3) a) 1 only b) 2 only c) 3 onlyd) 2 and 3e) All of the above 2. On the basis of intermolecular forces of attraction, rank the following three compounds in terms of increasing boiling point. H H H H H H H H C C O H H C C C H H C O C H H H H H H H H Ethanol Propane Dimethylether a) (lowest bp) Propane < Dimethyether < Ethanol (highest bp) b) (lowest bp) Propane < Ethanol < Dimethylether (highest bp) c) (lowest bp) Ethanol < Dimethylether < Propane (highest bp) d) (lowest bp) Ethanol < Propane < Dimethylether (highest bp) e) (lowest bp) Dimethylether < Ethanol < Propane (highest bp) 3. Nitrogen gas has very limited solubility in water. Under what condition(s) will the solubility of Nitrogen in water increase? a) At lower temperatures and higher pressure. b) At higher temperature only. c) At higher temperatures and lower pressure. d) At lower temperature only. e) At higher pressures only. 4. Which of the following molecular compounds would be highly soluble in toluene (see below)? (Remember: "Like dissolves Like".) a) Benzene only b) Naphthalene only c) Water only d) Benzene and Naphthalene e) Benzene, Naphthalene and Water 5. After carefully noting the orientation in which water surrounds each solute particle, which choice below best represents the true nature of how 2aCl exists in aqueous solution? Answer: a H O H H O H H O H H O H H O H H O O H H O O H H H O H H (a) Cl H Ca2+ Cl H (b) Cl H 2+ H H O O H H H H O O H H H H O O H H Ca H Cl O H H O H O H H O H H H O H H O H O O H H H H H H H H H H H O H H H H H O O H H O O H O O H H O O O H (c) CaCl2 (d) Ca2+ Cl2 (e) Ca H Cl O H H O O H 2 H H 2O H H O H H H O O H O H H O H O H H H H H H 6. How many grams of Oxygen, O are pre2ent in 3.6 x 10 molecules of O ? 2 Molar Mass(O ) 2 32.00 g/mol a) 5.4 x 10 g O b) 17 g O c) 1.9 g O 24 2 2 2 2 d) 1.2 x 10 g O 2 e) 6.0 x 10 g O 2 7. What is the molar mass for Sodium Sulfate? a) 55.06 g/mol b) 78.08 g/mol c) 126.05 g/mol d) 142.05 g/mol e) 215.13 g/mol 8. How many grams of iron are present in 75.0 grams of Fe O ? 2 3 MM(Fe O 2 3 159.70 g/mol a) 52.5 g of Iron b) 429 g of Iron c) 13.1 g of Iron d) 26.2 g of Iron e) 107 g of Iron o 9. A sample of Helium gas has a volume of 3.57 L at 25.0 C. What is the temperature of this gas (in degrees Celsius) at constant pressure when the volume expands to 6.42 L? a) 45.0 C b) 107 C c) 263 C d) 13.9 C e) 809 C 10. A sample of Nitrogen gas initially occupies a volume of 9.43 L at a pressure of 557 mm Hg. What would be the pressure (in mm Hg) of this same gas if the volume increases to 15.3 L? a) 1.11 x 10 mm Hg b) 343 mm Hg c) 3.86 mm Hg 4 d) 904 mm Hg e) 8.04 x 10 mm Hg 11. How many moles of Oxygen gas are present in a 4.55 L container held at 2.33 atm and 355 K? a) 0.364 moles O 2 b) 0.0176 moles O 2 c) 2.75 moles O 2 d) 4.58 x 10 moles O 2 e) 408 moles O 2 12. The partial pressure of oxygen, nitrogen and water in a gaseous mixture are 412 mm of Hg, 324 mm of Hg and 256 mm of Hg respectively. What is the percentage of oxygen in this mixture? a) 78.6 % O 2 b) 32.7 % O 2 c) 41.5% O 2 d) 25.8 % O 2 e) 58.5 % O 2 13. Which of the following three states of matter have an indefinite volume and an indefinite shape? 1) Solids 2) Liquids 3) Gases a) 1 only b) 2 only c) 3 only d) 1 and 2 e) All of the above 14. How would the Combined gas Law equation be rearranged to solve for a second temperature? Answer: b 15. What is the osmolarity of an aqueous 0.12 M Ba(NO ) solution? 3 2 a) 0.12 osmolar b) 0.24 osmolar c) 0.36 osmolar d) 0.60 osmolar e) 1.08 osmolar 16. Which phase change listed below represents the transition from the gaseous state to the solid state? a) Condensation b) Deposition c) Evaporation d) Freezing e) Sublimation 17. Which of the following phase changes listed below would be considered endothermic? 1) Freezing 2) Depositions 3) Evaporation a) 1 only b) 2 only c) 3 only d) 1 and 2 e) All of the above 18. The solubility limit for Potassium Chlorate at 70 C is 30.0 grams of KClO per 300 grams of water. What type of solution exists if 100.0 grams of KClO is di3 olved in 300 o grams of water at 70 C? a) Supersaturated solution b) Colloidal dispersion c) Saturated Solution d) Heterogeneous mixture e) Unsaturated solution 19. How many grams of KCl are required to prepare 42.0 mL of a 6.00 %(m/v) KCl solution? a) 0.397 g KCl b) 2.52 g KCl c) 7.00 g KCl d) 14.3 g KCl e) 252 g KCl 20. What volume (in mL) of a 0.655 M aqueous solution of glucose, C H O is requi6ed12o 6 provide 2.35 grams of C H O 6 12la6 Mass(C H O ) = 160.12 g6mol. a) 3.59 mL b) 19.9 mL c) 50.2 mL d) 117 mL e) 275 mL 21. Concentrated hydrochloric acid, HCl is 11.9 M. If 25.0 mL of 11.9 M HCl is diluted to a total volume of 100 mL, then what is the final concentration of the HCl solution? a) 0.0210 M b) 0.336 M c) 2.98 M d) 47.6 M e) 210 M 22. Which aqueous solution would be expected to have the lowest freezing temperature? a) 0.35 M NaBr b) 0.23 M Mg(NO ) 3 2 c) 0.70 M CH OH 3 d) 0.18 M FeCl 3 e) They would all be expected to have the same freezing temperature. 23. A cucumber is placed in a Brine solution and is converted to a pickle. What happens to the cucumber? a) The cucumber is placed in a hypotonic solution and it undergoes hemolysis. b) The cucumber is placed in a hypotonic solution and it undergoes crenation. c) The cucumber is placed in an isotonic solution and it undergoes hemolysis. d) The cucumber is placed in a hypertonic solution and it undergoes crenation. e) The cucumber is placed in a hypertonic solution and it undergoes hemolysis. 24. Helium has limited solubility in water. What pressure is required to maintain a solubility 2 o 4 of 2.50 x 10 M? k (HeH25 C = 3.70 x 10 M/atm 6 2 1 5 a) 9.25 x 10 atm b) 1.48 x 10 atm c) 6.76 x 10 atm d) 1.08 x 10 atm 25. What is the definition for part per billion, “ppb”? a) (grams of solute / grams of solution) x 10 9 b) (moles of solution / moles of solute) x 10 9 9 c) (moles of solute / moles of solvent) x 10 d) (grams of solute / grams of solvent) x 10 9 9 e) (grams of solvent / grams of solute) x 10 The equation below was balanced incorrectly. It should have been balanced as follows: 4 Fe (s) + 3 O 2g) 2 Fe O 2s)3 Assuming the coefficients that were given, the correct answers are provided redshaded below. Consider allowing Iron, Fe and Oxygen, O to react2to produce Fe O (rust) as2s3own below to answer the next three questions: 2 Fe (s) + 3 O 2(g) Fe O 2(s3 26. Which substance is the limiting reactant when 0.95 moles of Iron, Fe and 0.65 moles of oxygen, O a2e allowed to react as shown in the reaction above? a) Fe b) O 2 c) Fe 2 3 d) None of these; they are mixed in exact proportions. 27. What is the percentage yield in a certain experiment, if 0.18 moles of Fe O were 2 3 recovered at the end of the reaction when 0.95 moles of Iron, Fe and 0.65 moles of oxygen, O a2e allowed to react as shown in the reaction above? a) 19 % b) 28 % c) 38 % d) 68 % e) 83 % 28. How many grams of iron, Fe is required to react with 15.0 grams of Oxygen, O ? 2 Molar Mass(O ) =2 32.00 g/mol and Molar Mass(Fe) = 55.85 g/mol a) 5.73 g Fe b) 8.59 g Fe c) 17.5 g Fe d) 26.2 g Fe e) 39.3 g Fe 29. Acetic acid is added to water to make vinegar. Which of the following Colligative properties are observed? a) The vapor pressure of the vinegar solution is lower than pure water. b) The boiling temperature of the vinegar solution is higher than pure water. c) The freezing temperature of the vinegar solution is lower than pure water. d) The osmotic pressure of the vinegar solution is greater than pure water. e) All of these properties are observed.
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