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by: Hannah B.


Marketplace > Auburn University > Chemistry > CHEM 1040 > CHEM 1040 EXAM ONE
Hannah B.
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Compilation of questions from the book, from class, and from myself. Great study tool for chapters 7.3, 12-14 from Atoms First textbook.
Fundamental Chemistry II
Ria Astrid Yngard
Study Guide
Chemistry, Yngard, CHEM 1040, Fundamentals of Chemistry, Atoms First, Fundamentals of Chemistry II, Fundamentals of Chemistry 2, exam
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This 6 page Study Guide was uploaded by Hannah B. on Thursday February 4, 2016. The Study Guide belongs to CHEM 1040 at Auburn University taught by Ria Astrid Yngard in Winter 2016. Since its upload, it has received 425 views. For similar materials see Fundamental Chemistry II in Chemistry at Auburn University.


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Date Created: 02/04/16
CHEM 1040 EXAM 1 1. Calculate the amount of heat required to convert 1.00 mole of ice at -11ºC to steam at 115ºC under constant pressure. Sice = 2.03 J/gºC Swater = 4.18 J/gºC Ssteam = 1.99 J/gºC Hfusion = 6.01 kJ/mole Hvaporization = 40.79 kJ/mole 2. Consider the following reaction at 298 K: Calculate ΔS ,sys surr and ΔS univor the reaction. 3. The vapor pressure of liquid X is lower than that of liquid Y at 20°C, but higher at 60°C. What can you deduce about the relative magnitude of the molar heats of vaporization of X and Y? 4. Calculate the amount of heat needed to boil 29.5g ethanol (C H O2,6beginning from a temperature of -95.7ºC. Boiling point of ethanol: 78.29ºC Heat capacity of ethanol: 2.238 J/gK Hvap: 38.56 kJ/mol 5. Calculate the molality of each of the following solutions: (a) 14.3 g of sucrose (C12 22) i11 685 g of water, (b) 7.15 moles of ethylene glycol (C H2 6) 2n 3505 g of water. 6. How does the entropy of a system change for each of the following processes? (a) heating bromine from 30ºC to 80ºC (b) CO 2s) —> CO (g2 (c) 2NO(g) + O (2) —> 2NO (g)2 (d) dissolution of a solute in sugar (e) decrease in volume Page 1 of 6 7. Calculate the % mass of NaCl in a solution of 3.50g NaCl in 75.0g H O. 2 8. Calculate ΔS sys for (a) the isothermal compression of 0.0050 mole of an ideal gas from 112 mL to 52.5 mL, (b) the isothermal compression of 0.015 mole of an ideal gas from 225 mL to 22.5 mL, and (c) the isothermal expansion of 22.1 moles of an ideal gas from 122 L to 275 L. 9. Find the temperatures at which reactions with the following ΔH and ΔS values would become spontaneous: (a) ΔH = −126 kJ/mol, ΔS = 84 J/K · mol; (b) ΔH = −11.7 kJ/mol, ΔS = −105 J/K · mol. 10. A 2.6-L sample of water contains 192 μg of lead. Does this concentration of lead exceed the safety limit of 0.050 ppm of lead per liter of drinking water? 11. A commercial bleaching solution contains 3.62% by mass sodium hypochlorite, NaOCl. What is mass (g) of NaOCl in a bottle containing 2.50kg of bleaching solution? 12. What pressure of CO is2required to keep the CO conc2ntration in a bottle of club soda at 0.12M at 25ºC? k(co ): 3.4 x 10^-2 mol/L•atm at 25ºC 2 Page 2 of 6 13. Calculate the heat required to melt 43.7g of benzene to a temperature of 78.3. melting point of benzene: 5.49ºC benzene heat capacity: 1.63 J/gK Hfus: 9.87 kJ/mol 14. What is the formula of Raoult’s Law? 15. A solution of 6.85 g of a carbohydrate in 100.0 g of water has a density of 1.024 g/mL and an osmotic pressure of 4.61 atm at 20.0°C. Calculate the molar mass of the carbohydrate. 16. Define (a) viscosity, (b) dynamic equilibrium, (c) vapor pressure, (d) triple point, (e) solubility. 17. How much heat (in kJ) is needed to convert 866 g of ice at −15°C to steam at 146°C? (The specific heats of ice and steam are 2.03 and 1.99 J/g · °C, respectively.) 18. Describe endothermic vs. exothermic. 19. The vapor pressure of pure water at 108ºC is 1004 torr. An aqueous solution of ethylene glycol and water has a vapor pressure of 1.10 atm at 108ºC. Assuming Raoult’s Law is obeyed, what is the mole fraction of ethylene glycol in this solution? 1 atm = 760 torr Page 3 of 6 20. What is the tyndall effect? 21. A solution is prepared by condensing 4.00 L of a gas, measured at 27°C and 748 mmHg pressure, into 75.0 g of benzene. Calculate the freezing point of this solution. 22. What is the Van’t Hoff factor of NaCl in an aqueous solution? 23. Which of the following properties indicates very strong intermolecular forces in a liquid: (a) very low surface tension, (b) very low critical temperature, (c) very low boiling point, (d) very low vapor pressure? 24. The standard enthalpy of formation of gaseous molecular iodine is 62.4 kJ/mol. Use this information to calculate the molar heat of sublimation of molecular iodine at 25°C. 25. A student dissolves 1.5g of ammonia in 200mL of a solvent with a density of 0.94g/ml. Volume doesn't change when ammonia dissolves. Calculate the molarity and molality of the ammonia. 26. A chemist mixes 32g of ethanol with 42g of 4-methyl-2-pentanone and 56g of acetic acid. Calculate the percent by mass for each. Page 4 of 6 27. 129mg of an unknown protein are dissolved in enough solvent to make a 5.00mL solution. The osmotic pressure of this solution is measured be 0.313atm at 25ºC. Calculate the molar mass of the protein. R=0.08206 atm•L/mol•K -3 28. At 25ºC the Henry’s Law constant for PH ga3 in water is 8.1 x 10 M/atm. Calculate the mass in grams of PH ga3 that can be dissolved in 625mL of water at 25ºC and a PH partial3 pressure of 1.07atm. 29. At a certain temperature the vapor pressure of C7H16 is 472mmHg. Suppose a solution is made by mixing 144g of C7H16 and 144g of CH3COBr. Calculate the partial pressure of C7H16 vapor. 30. Describe the 3 ways molecules move. 31. The molar heats of fusion and vaporization of benzene are 10.9 and 31.0 kJ/mol, respectively. Calculate the entropy changes for the solid-to-liquid and liquid-to-vapor transitions for benzene. At 1 atm pressure, benzene melts at 5.5°C and boils at 80.1°C. The melting point of benzene is 5.5 + 273.15 = 278.7 K and the boiling point is 80.1 + 273.15 = 353.3 K. 32. According to Table 14.4, a reaction will be spontaneous only at high temperatures if both ΔH and ΔS are positive. For a reaction in which ΔH = 199.5 kJ/mol and ΔS = 476 J/K · mol, determine the temperature (in °C) above which the reaction is spontaneous. Page 5 of 6 1. q=55.3 2. ΔS sys= −327.2 J/K · mol; ΔS surr 1918 J/K · mol; ΔS univ 1591 J/K · mol 3. Liquid X has a larger ΔH vapthan does liquid Y. 4. 36.2 kJ 5. (a) 0.0610 m (b) 2.04 m 6. (a) increase (b) increase (c) decrease (d) increase (e) decrease 7. 4.46% NaCl 8. (a) −0.031 J/K (b) −0.29 J/K (c) 1.49 × 10 J/K 9. (a) all temperatures (b) below 111 K 10. Yes 11. 90.5g NaOCl 12. 3.5 atm 13. 11.5 kJ 14. Psolvent = Xsolvent•Pºsolvent 15. 342 g/mol 16. (a) a measure of a fluid’s resistance to flow, (b) liquid molecule evaporate and vapor molecule condense at the same rate, (c) the pressure exerted when liquid and vapor states are in dynamic equilibrium, (d) combination of pressure and temperature where three phases of a substance exist in equilibrium, (e) amount of solute dissolved in a given volume of a saturated solution at a specific temperature 17. 2.72 × 10 kJ 18. An endothermic reaction occurs when energy is absorbed from the surroundings in the form of heat (positive ΔH). Conversely, an exothermic reaction is one in which energy is released from the system into the surroundings (negative ΔH). 19. 0.167 atm 20. light shines through a colloidal solution 21. −5.4°C 22. 2 23. (d) very low vapor pressure 24. 62.4 kJ/mol 25. Molarity = 0.44037M molality = 0.47225m 26. ethanol: 24.6% 4-methyl-2-pentanone: 32.3% acetic acid: 43.1% 27. 2.0167 x 10 g/mol 28. 0.18416g 29. 260.047 mmHg 30. translational: entire molecule from one place to another / rotational: rotation about an axis / vibrational: motion within a molecule 31. melting: 39.1 J/K•mol / boiling: 87.7 J/K•mol 32. 146ºC Page 6 of 6


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