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Practice Exam 2

by: Kyle A. Headen

Practice Exam 2 CHEM 1307

Kyle A. Headen

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Help get a feel what the Second Exam gives you all. If you feel confident in yourself you won't need it otherwise this is just for extra practice.
Experimental Principles of Chemistry 1
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This 7 page Study Guide was uploaded by Kyle A. Headen on Monday October 17, 2016. The Study Guide belongs to CHEM 1307 at Texas Tech University taught by Whittlesey in Fall 2016. Since its upload, it has received 11 views. For similar materials see Experimental Principles of Chemistry 1 in Chemistry at Texas Tech University.

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Date Created: 10/17/16
CHEM 1307 Fall Semester 2016 Practice Exam 2 1. An experiment shows that a 389 mL gas sample has a mass of 0.236 g at a pressure of 713 mmHg and a temperature of 29.00 °C. What is the molar mass of the gas? a. 16.04 g/mol b. 17.03 g/mol c. 18.02 g/mol d. 13.83 g/mol e. 20.01 g/mol 2. Which products are expected from the reaction of sodium carbonate and hydrochloric acid: a) NaClO 4 b) H O 2 c) CO 2 d) b and c e) all of the above 3. Considering the following reaction at 298 K: Zn (s) + 2HCl (aq) à ZnCl (2q) + H (g2 If 456 mL of gas are collected over water and the atmospheric pressure (total pressure) is 0.987 atm, what is the partial pressure of H in the collected gas? The vapor pressure of H O at 298 K is 23.78 2 2 mmHg. a) 0.0313 atm b) 750. mmHg c) 22.793 mmHg d) 0.987 atm e) 0.956 atm 4. A chemical reaction has the equation: 2A + B →C. In which case is B the limiting reactant? a) I b) II c) III d) IV e) none of these 5. A 17.0-g sample of HF is dissolved in water to give 2.0 × 10 mL of solution. The concentration of the solution is: a) 0.85 M b) 0.17 M c) 0.09 M d) 4.2 M e) 8.5 M 6. What volume of 18 M sulfuric acid must be used to prepare 1.80 L of 0.215 M H SO ?2 4 a) 22 mL b) 0.39 mL 3 c) 2.2 × 10 mL d) 4.3 mL e) 7.0 mL 7. You have two solutions of sodium chloride. One is a 2.00 M solution, the other is a 4.00 M solution. You have much more of the 4.00 M solution and you mix the solutions together. Which of the following could be the concentration of the final solution? a) 2.50 M b) 3.00 M c) 3.70 M d) 6.00 M e) 7.50 M 8. 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. 9. When solutions of strontium chloride and sodium carbonate react, which of the following are spectator ions? a) strontium ions and sodium ions b) sodium ions and chloride ions c) sodium ions and carbonate ions d) strontium ions and carbonate ions e) chloride ions and carbonate ions 10. With what volume of 5.00 M HF will 3.95 g of calcium hydroxide react completely, according to the following reaction? 2HF + Ca(OH) → 2 2 2 2H O a) 10.7 mL b) 107 mL c) 533 mL d) 21.3 mL e) 46.9 mL – 11. The oxidation number of iodine in IO 2 is: a) –1 b) +3 c) –3 d) +5 e) –5 12. In the reaction P4(s) + 10Cl2(g) → 4PCl (5), the reducing agent is a) Cl 2 b) PCl 5 c) P 4 – d) Cl e) none of these 13. A gas sample is held at constant pressure. The gas occupies 3.62 L of volume when the temperature is 21.6°C. Determine the temperature at which the volume of the gas is 3.45 L. a) 309 K b) 281 K c) 20.6 K d) 295 K e) 554 K 14. You are holding four identi cal balloons each containing 10.0 g of a different gas at the same temperature and pressure. The balloon containing which gas is the largest balloon? a) H 2 b) He c) Ne d) O 2 e) All have the same volume. 15. A gas sample is heated from -20.0°C to 57.0°C and the volume is increased from 2.00 L to 4.50 L. If the initial pressure is 0.109 atm, what is the final pressure? a) 0.0371 atm b) –0.138 atm c) 0.320 atm d) 0.188 atm e) 0.0632 atm 16. A sample of oxygen gas has a volume of 3.52 L at 27°C and 800.0 torr . How many oxygen molecules does it contain? (760 torr = 1 atm) 22 a) 9.06 × 10 b) 6.88 × 10 25 24 c) 1.01 × 10 d) 4.00 × 10 24 26 e) 7.66 × 10 17. Which gas has the highest density if all gases are under the same conditiof pressure, volume, temperature and number of mols? a) He b) Cl 2 c) CH 4 d) NH 3 e) all gases have the same density 18. Gaseous C H reacts with O according to the following equation: 2 4 2 CH2 4 gOg( 2 2CO(g+HO2( ) 2 What volume of oxygen gas at a temperature of 0°C and a pressure of 1.00 atm is needed to react with 5.06 mol of C2H 4 a) 15.2 L b) 37.8 L 2 c) 3.40 × 102L d) 1.13 × 10 L e) Not enough information is given to solve the problem. 19. A gaseous mixture containing 1.5 mol Ar and 3.5 mol CO 2has a total pressure of 7.5 atm. What is the partial pressure of CO ? 2 a) 2.3 atm b) 1.4 atm c) 18 atm d) 5.3 atm e) 7.5 atm 20. What would happen to the average kinetic energy of the molecules of a gas sample if the temperature of the sample increased from 20°C to 40°C? a) It would double. b) It would increase. c) It would decrease. d) It would become half its value. e) Two of these. 21. Which of the following would have a higher rate of effusion than 2H2? a) N 2 b) O 2 c) Cl2 d) CH 4 e) CO 2 22. Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions o2 K S and Fe(NO ) are mixed. 3 2 A) K (aq) + NO (a3) → KNO (s) 3 B) Fe 2+(aq) + S (aq) + 2 K (aq) + 2 NO (3q) → FeS(s) + 2 K (aq) + 2 NO (aq) 3- C) Fe 2+(aq) + S (aq) + 2 K (aq) + 2 NO (3q) → Fe 2+(aq) + S (aq) + 2 KNO (3) 2+ 2- D) Fe (aq) + S (aq) → FeS(s) E) No reaction occurs. 23. A 300.0 mL flask contains pure helium at a pressure of 539 torr. A second flask with a volume of 450.0 mL contains pure argon at a pressure of 896 torr. If the two flasks are connected through a stopcock and the stopcock is opened, what is the total pressure? a. 1.41 x 10 torr b. 682 torr c. 753 torr d. 1.70 x 10 torr e. 718 torr 24. The following is an example of which type of reaction: CH2 4 gOg( 2 2CO(g→2H2 ( ) 2 a. precipitation b. combustion c. oxidation-reduction d. b and c e. all of the above 25. Which of the following represent a unit for pressure: 2 a. Pascal (N/m ) b. atmosphere c. pounds per square inch (psi) d. mm-Hg e. all of the above 26. Calculate the mass percent composition of lithium in Li PO .3 4 a) 55.27% b) 26.75% c) 30.72% d) 26.75% e) 17.98% 27. You take an aspirin tablet (a compound consisting solely of carbon, hydrogen, and oxygen) with a mass of 1.00 g, combust it under an oxygen atmosphere, and collect 2.20 g of carbon dioxide and 0.400 g water. The molar mass of aspirin is between 170 and 190 g/mol. The molecular formula of aspirin is a) C 6 8 5 b) C 9 8 4 c) C 8 10 5 d) C 10O6 4 e) none of these 28. What is the coefficient for water when the following equation is balanced in standard form? As(OH) (s) + H SO (aq) → As (SO ) (aq) + H O(l) 3 2 4 2 4 3 2 a) 1 b) 2 c) 4 d) 6 e) 12 29. Which substance is the limiting reactant when 2.0 g of sulfur reacts with 3.0 g of oxygen and 4.0 g of sodium hydroxide according to the following chemical equation: 2 S(s) + 3 O2(g) + 4 NaOH(aq) → 2 Na 2O (4q) + 2 H O2l) A) S(s) B) NaOH(aq) C) O2(g) D) H2O E) None of these substances is the limiting reactant. CHEM 1307 Fall Semester 2016 Practice Exam 2 Answer Key Question Answer 1 A 2 D 3 E 4 B 5 D 6 A 7 C 8 C 9 B 10 D 11 B 12 C 13 B 14 A 15 E 16 A 17 B 18 C 19 D 20 B 21 D 22 D 23 C 24 D 25 E 26 E 27 B 28 D 29 B


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