KEEP THIS SECTION!!!!!!!!!
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1 KEEP THIS SECTION!!!!!!!!! CHEMISTRY 202 Hour Exam II (Multiple Choice Section) November 1, 2018 Dr. D. DeCoste Name Signature T.A. This exam contains 20 questions on 5 numbered pages. Check now to make sure you have a complete exam. Determine the best answer to these questions and enter these on the special answer sheet. Also, circle your responses in this exam booklet. Each multiple choice question is worth 3 points (total of 60 points). The free response section is worth a total of 60 points. Useful Information: Always assume ideal behavior for gases (unless explicitly told otherwise). 760 torr = 1.00 atm R = Latm/molK = J/Kmol K = C NA = x E = q + w S = qrev/t H = E + PV G = H TS Here are some of the formulas we used/derived in studying thermodynamics. An individual formula may or may not apply to a specific problem. This is for you to decide! S = nrln(v2/v1) S = H/T Cv = (3/2)R Cp = (5/2)R S = ncln(t2/t1) G = G + RTln(Q) Ssurr = q/t w = P V qrev = nrtln(v2/v1) q = nc T ln(k) = H R 1 T + S R K ln K 2 1 H = R 1 T2 1 T 1
2 Hour Exam II (Multiple Choice Section) Page No In lecture I showed how the kinetic molecular theory applies to solids by heating a brass sphere and showing that this caused it to expand. I then cooled the sphere by sticking it in ice. Suppose the brass sphere had a mass of 50.0 g and that I heated it to in the Bunsen burner. If I placed the sphere in g of ice at 10.0, which of the following best describes what happened to the ice? Assume that no heat is transferred to the air (that is, all heat is transferred from the sphere to the ice), and that heat capacities are independent of temperature. Heat capacity of brass: J/gK Heat capacity of ice: 2.03 J/gK Heat capacity of liquid water: 4.18 J/gK Enthalpy of fusion of ice at 0 : 6.01 kj/mol a) None of the ice melted and we end up with ice at 1.4. b) Some of the ice melted; specifically, 1.31 g of ice melted. c) Some of the ice melted; specifically, 23.7 g of ice melted. d) All of the ice melted and we end up with water at 3.8. e) All of the ice melted and we end up with water at You carry out an acid-base reaction in a Styrofoam cup calorimeter by mixing aqueous solutions of HCl and NaOH, measuring the temperature change (which is positive), and determining ΔH for the reaction in kj/mol. Your lab partner carries out the same reaction in a bomb calorimeter, measures the temperature change (also positive), and determines ΔE for the reaction in kj/mol. Which of the following best describes the relationship between ΔH and ΔE? a) The values for ΔH and ΔE are both negative and the magnitude of the value for ΔH is much greater than the value for ΔE. b) The values for ΔH and ΔE are both positive and the magnitude of the value for ΔH is much greater than the value for ΔE. c) The values for ΔH and ΔE are both positive and the magnitude of the value for ΔE is much greater than the value for ΔH. d) The values for ΔH and ΔE are both positive and the magnitudes of the value for ΔH and ΔE do not differ significantly. e) The values for ΔH and ΔE are both negative and the magnitudes of the values for ΔH and ΔE do not differ significantly. 3. Weather in Illinois is a lot of fun -- it snowed on the day of the Homecoming Parade! While the ground temperature was above freezing, the temperature at higher altitudes was low enough for the formation of snow. So, let s suppose that a 1.00 g snowflake (made of pure water) at 0.0 fluttered its way toward campus and melted while surrounded by a constant temperature of 2.0. Determine Suniv for the process of the snowflake melting. The enthalpy of fusion of ice at 0 is 6.01 kj/mol a) 1.22 J/K b) 0.01 J/K c) 1.21 J/K d) 1.22 J/K e) 2.43 J/K 4. In an isothermal free expansion of an ideal, monatomic gas, how many of the following are equal to zero? H, E, w, q, S, Ssurr, Suniv, G a) 2 b) 3 c) 4 d) 5 e) 6
3 Hour Exam II (Multiple Choice Section) Page No. 2 5,6. A classic thermochemistry lab involves looking at the relationships of ΔH for the following three reactions: 1. Na2CO3(s) + 2HCl(aq) 2NaCl(aq) + CO2(g) + H2O(l) 2. NaHCO3(s) + HCl(aq) NaCl(aq) + CO2(g) + H2O(l) 3. 2NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(l) For this problem, you will determine the value of ΔH for the first reaction and the expected temperature change of the second reaction. In both cases you react g solid with ml of 1.00M HCl (the density of the HCl solution is 1.00 g/ml and the HCl is in excess). Assume the solutions have a heat capacity of 4.18 J/g and that ΔH values are constant over the temperature changes in question. 5. In reaction #1 (between sodium carbonate and HCl), you record the temperature of the solution as increasing from 28.1 to Determine ΔH for reaction #1 in units of kj/mol sodium carbonate a) 543 kj/mol b) 27.7 kj/mol c) 27.7 kj/mol d) 28.8 kj/mol e) 28.8 kj/mol 6. In reaction #2 (between sodium bicarbonate and HCl), you start with the HCl solution at Given that ΔH for the decomposition of baking soda as written above (reaction #3) is 85.5 kj, determine the expected final temperature when reacting NaHCO3(s) and HCl(aq). a) 21.8 b) 24.9 c) 28.0 d) 31.1 e) ,8. In another classic thermochemistry lab you heat a block of metal in a boiling water bath and then place it in a coffee-cup calorimeter containing room temperature water. Suppose you heat 50.0 g of aluminum metal (specific heat capacity = J/g C) in a boiling water bath (100 C) and quickly transfer it to g of water (specific heat capacity = 4.18 J/g C) at 25.0 C in a Styrofoam calorimeter. Assume there is no heat loss to the surroundings in the time it takes to reach thermal equilibrium (same temperature of metal and water) and that the specific heat capacities are independent of temperature. 7. Determine the temperature of the water at thermal equilibrium. a) 15.9 b) 25.0 c) 28.0 d) 32.3 e) Determine ΔSuniv for the process of the metal and water reaching thermal equilibrium. a) 1.09 J/K b) J/K c) J/K d) J/K e) J/K
4 Hour Exam II (Multiple Choice Section) Page No Consider the isothermal expansion and compression of an ideal gas. There is one mole of gas in a container fitted with a piston and the expansion is carried out in such a way as to produce the maximum work possible. The compression is done to minimize the work required. What is the ratio (R) of work during the expansion to work during the compression? That is, wwwwwwww dddddddddddd tthee eeeeeeeeeeeeeeeeee wwwwwwww dddddddddddd tthee cccccccccccccccccccccc = R a) R < 1 b) R = 1 c) 1 < R < 1 d) R = 1 e) R > In how many of the following cases is q 0? I. An isothermal expansion of an ideal gas against a constant external pressure. II. An isothermal reversible expansion of an ideal gas against a constant external pressure. III. An isothermal free expansion of an ideal gas. IV. An isothermal phase change between a liquid and a vapor at its boiling point. V. A chemical reaction carried out at constant temperature. a) 1 b) 2 c) 3 d) 4 e) Consider two containers of ideal, monatomic gases (both equimolar, with the same volume, and initially at the same pressure and temperature). Container 1 is a fixed volume container, and container 2 is fitted with a frictionless, massless piston. You double the temperature in container 1. In order for S to be the same in each container, by what factor do you change the temperature in container 2? a) 1.52 b) 1.67 c) 2.00 d) 2.83 e) In which of the following spontaneous cases will Suniv and G have the same sign? a) None the signs for Suniv and G are always opposite for spontaneous processes. b) A spontaneous phase change at constant pressure and temperature. c) A spontaneous chemical reaction at constant pressure and temperature. d) A spontaneous isothermal expansion of an ideal gas. e) A spontaneous isothermal compression of an ideal gas. 13. The reaction N2(g) +3H2(g) 2NH3(g) is spontaneous at a given temperature. Suppose you have a mixture of these gases at equilibrium at this temperature. How will heating the gas mixture affect the equilibrium position? a) It will shift to the right. b) It will shift to the left. c) It will not shift. d) There is no way to tell.
5 Hour Exam II (Multiple Choice Section) Page No. 4 14, 15. Consider the two-bulb container systems we have discussed. In this case you have the same number of moles of helium and neon (assume both are ideal, monatomic gases). The helium is initally in one bulb (with a volume of 2.0 L) and the neon is in the other bulb (with a volume of 6.0 L). Both gases are initially at 25 and you quickly heat the neon to 35 and then open the stopcock, allowing the gases to mix. Assume this two-bulb container is insulated from the surroundings as the gases mix and reach thermal equilibrium. 14. Which of the following factors contributes most to the overall spontaneity of the process that occurs once the valve is opened? a) The He mixing throughout the container. b) The Ne mixing throughout the container. c) The He reaching thermal equilibrium. d) The Ne reaching thermal equilibrium. e) At least two of the above equally contribute the most to the spontaneity. 15. Do any of the following factors contribute negatively to Suniv? a) Yes, the Ne mixing throughout the container. b) Yes, the He mixing throughout the container. c) Yes, the Ne reaching thermal equilibrium. d) Yes, the He reaching thermal equilibrium. e) No, none of the above factors (a-d) contribute negatively to Suniv One mole of a monatomic ideal gas (for which S = 8.00 J/K at 73.0 C) is heated at a constant pressure from 73.0 C to 27.0 C. Determine the following values: 16. H 17. S 18. G a) 0 b) 831 J c) 1.25 kj d) 1.25 kj e) 2.08 kj a) 0 b) 3.37 J/K c) 5.06 J/K d) 8.43 J/K e) J/K a) 0 b) 831 J c) 1.25 kj d) 1.25 kj e) 2.08 kj
6 Hour Exam II (Multiple Choice Section) Page No. 5 19, 20. Consider the reaction 4NO2(g) + O2(g) 2N2O5(g) at 25.0 C and the following data: H f (kj/mol) NO2(g) 33.2 N2O5(g) Determine the value of ΔH for the reaction as written. a) 21.9 kj/mol b) 21.9 kj/mol c) kj/mol d) kj/mol e) kj/mol 20. Assuming ΔH values are independent of temperature, by what factor does the value of the equilibrium constant change for the reaction as written if we change the temperature from 25.0 C to 30.0 C? a) b) c) 1.00 d) 1.16 e) 2.08
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