Chemistry 104 Practice Final Exam - Chemistry 104 Practice...

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Chemistry 104 Practice Final Exam True/False 1. All exothermic reactions are spontaneous. 2. At constant volume, E = q. 3. Doubling the coefficients of a balanced chemical reaction will double the H of the reaction. 4. The standard entropy of argon gas is greater than the standard entropy of CO 2 (g). 5. The change in free energy ( G) for the process H 2 O (s) → H 2 O (l) occurring at exactly 0 o C is exactly equal to zero. 6. The enthalpy change for the reaction: N 2 (g) + O 2 (g) → 2NO(g) is the same as the enthalpy change for the sum of the following reactions: N 2 (g) +O 2 (g) →2NO 2 (g) NO (g) +O 2 (g) →NO 2 (g) 7. Suppose that 19.15 L of an ideal, monatomic gas, has an initial pressure of 3.0 atm. It expands against a constant external pressure of 1 .0 atm., until the volume is doubled. There is no exchange of heat between the system and the surroundings. Calculate E for this process. a) +1.94 x 10 3 J b) +5.8 x 10 3 J c) -1.94 x 10 3 J d) + 579.5 J e) -19.15 J 8. For a particular process, q = -20 kJ and w = 15 kJ. Which of the following statements is true? a) Heat flows from the system to the surroundings. b) The system does work on the surroundings. c) E = -35 kJ d) all of the above (a-c) are true. e) none of the above (a-c) are true. 9. 100 mL of water was placed in a coffee cup calorimeter. The initial temperature was 21.6 o C. One gram of ammonium nitrate was added to the water. After the solid dissolved, the final temperature of the solution was 20.5 o C. The dissolving of this solid is a process: a) that has H < 0 b) that has G > 0 c) that has S universe < 0 d) that has S < 0 e) none of the above (a-d)
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10. Assuming that the heat capacity of the solution is the same as the heat capacity of water (4.184 J/g o C), calculate the H for the dissolution of ammonium nitrate and express it a kJ/mol. (m.w. Ammonium Nitrate = 80 g/mol) a) -0.42 kJ/mol b) +0.42 kJ/mol c) -37.2 kJ/mol d) +37.2 kJ/mol e) +67.5 kJ/mol 11. Consider the reaction: C 2 H 5 OH (l) + 3O 2 (g → 2CO 2 (g) + H 2 O (l) When a 15.1 g sample of ethanol (MW = 46.1 g/mol) is burned, 4.49 x 10 2 kJ of energy are released. How much energy is released when 0.65 mol of ethanol are burned? a) 891 kJ b) 1370 kJ c) 2109 kJ d) 89.7 kJ e) 255 kJ 12. For the combustion of ethanol as described in the equation above, which of the following statements is/are true? 1. The reaction is endothermic
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This note was uploaded on 05/20/2008 for the course CHEM 104 taught by Professor Yerkes during the Spring '08 term at University of Illinois at Urbana–Champaign.

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Chemistry 104 Practice Final Exam - Chemistry 104 Practice...

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