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CHEM 1151 General Chemistry for Engineers




F11 CHEM 1151 Midterm Exam 2 (Ver A).doc Download Attachment;NAME (LAST, FIRST);CHEM 1151 General Chemistry for Engineers;Fall 2011;MIDTERM EXAM 2, VERSION A;RECITATION SECTION (Please circle both name of TA & Day/Time);TA;Day/Time;TA;Day/Time;M 2:50-4:30 PM;M 2:50-4:30 PM;Tu 8:00-9:40 AM;Tu 11:45 AM-1:25 PM;Lisa;Ryan;Hawver Tu 9:50-11:30 AM;Pavlicek Tu 1:35-3:15 PM;Tu 11:45 AM-1:25 PM;W 2:50-4:30 PM;M 11:45 AM-1:25 PM;Th 11:45 AM-1:25 PM;Tu 9:50-11:30 AM;F 8:00-9:40 AM;Chris;Dave;Toher;Murison F 9:50-11:30 AM;Tu 1:35-3:15 PM;Tu 3:25-5:05 PM;F 1:35-3:15 PM;Please make sure that the following information is in pencil on the bubble sheet (Scantron);1) Your name (last, first) and 9-digit student ID number (fill in bubbles under ID number);2) 1151 for course number;3) Version of Exam (A) (write at top of Scantron);4) Fill in the bubble for question 15 with your version of the exam (A);The exam is divided into two sections;Section I: Multiple-choice questions: 14 questions worth 5 pts each, no penalty for;guessing but also no partial credit. Circle your answer to each question and transfer;these answers to your bubble sheet.;Section II: Open-response questions: No credit for guessingyou must show all correct;work to receive full creditbut partial credit will be awarded for incomplete correct;work! Points may be deducted for incorrect use of significant figures. Show all work;clearly and concisely in space provided & box your final answer.;A separate handout provides useful constants, definitions, conversion factors, equations, and;tables for your reference.;Section;Score;Multiple-choice questions;correct 5 = ____/70;Open-response question 15;/10;Open-response question 16;/10;Open-response question 17;/10;Total;/100;CHECK TO MAKE SURE THIS DOCUMENT CONTAINS 8 PAGES;CHEM 1151 General Chemistry for Engineers;Fall 2011;Section A: Multiple-choice questions (5 pts each);Circle your answer to each question;1. How many of the following molecules can participate in hydrogen bonding?;A);B);C);D);E);1;2;3;4;5;2. Which one of the following materials is expected to have the largest band gap?;A);B);C);D);E);A metal;A metalloid;A conductor;A semiconductor;An insulator;3. By how much faster does N2(g) effuse than Br2(g) at a common temperature?;A);B);C);D);E);N2(g) effuses 0.175 times as fast as Br2(g);N2(g) effuses 0.419 times as fast as Br2(g);N2(g) effuses 1.75 times as fast as Br2(g);N2(g) effuses 2.39 times as fast as Br2(g);N2(g) effuses 5.71 times as fast as Br2(g);4. Which one of the following compounds would you expect to have the lowest normal boiling;point?;A);B);C);D);E);CH4;CH3OH;CH3Cl;CCl4;CH2Cl2;2;CHEM 1151 General Chemistry for Engineers;Fall 2011;5. According to the phase diagram depicted below for carbon dioxide (not drawn to scale);which one of the following statements is false?;A);B);C);D);E);The melting point of solid CO2 is near 216 K between 5.1 and 72.9 atm.;CO2 cannot exist in the liquid phase at pressures below 5.1 atm.;The normal boiling point of CO2 is 78.5 C.;Liquid and gaseous CO2 cannot coexist in equilibrium at temperatures above 31 C.;There is only one temperature and pressure at which solid, liquid, and gaseous CO 2 can;coexist at equilibrium.;6. A crystal does not conduct electricity, is hard and brittle, and melts at a relatively high;temperature. Both the melt (liquid state) for this crystal and an aqueous solution of this;crystal conduct electricity. What is the type of crystal?;A);B);C);D);E);An ionic crystal;A metallic crystal;A network covalent crystal;A molecular crystal;An amorphous crystal;7. How much pure water must be added to 100. mL of a 3.00 M aqueous solution to dilute its;concentration to 0.500 M?;A);B);C);D);E);30.0 mL;60.0 mL;100. mL;500. mL;600. mL;3;CHEM 1151 General Chemistry for Engineers;Fall 2011;8. Which one of the following aqueous solutions is the worst conductor of electricity?;A);B);C);D);E);1 M 1-propanol;1 M potassium iodide;1 M butanoic acid;1 M sodium sulfate;They all conduct electricity equally well;9. An aqueous solution of an unknown dilute solute has a freezing point of -0.520 C. If water;has a cryoscopic constant of Kf = 1.86 C/m and an ebullioscopic constant of;Kb = 0.512 C/m, what is the change in the normal boiling point of this solution relative to;pure water?;A);B);C);D);E);-1.86 C;0.143 C;0.512 C;1.86 C;1.88 C;10. What is the sum of the stoichiometric coefficients when the following equation is balanced;with smallest integer coefficients?;NaOH(aq) + NaNO2(aq) + Al(s) + H2O(l) NH3(aq) + NaAlO2(aq);A);B);C);D);E);6;7;8;9;10;11. What happens when an aqueous solution of CrCl2 is mixed with an aqueous solution of;Li2CO3?;A);B);C);D);E);Nothing happens (i.e., no precipitation occurs);Both CrCO3(s) and LiCl(s) precipitate;LiCl(s) precipitates;LiCl2(s) precipitates;CrCO3(s) precipitates;4;CHEM 1151 General Chemistry for Engineers;Fall 2011;The following information applies for Questions 12 & 13;Consider the decomposition of potassium chlorate;2 KClO3(s) 2 KCl(s) + 3 O2(g);12. How many grams of KClO3 are required to produce a theoretical yield of 8.5 g of KCl?;A);B);C);D);E);8.5 g;14. g;17. g;23. g;46. g;13. What is the percent yield if 1.7 g of potassium chloride actually is produced and the;theoretical yield is 8.5 g?;A);B);C);D);E);6.0%;10. %;11. %;20. %;33. %;14. What is the work when a gas is compressed from 20.0 L to 10.0 L with a constant external;pressure of 5.00 atm?;A);B);C);D);E);-5.06 kJ;-5.00 kJ;3.33 kJ;5.00 kJ;5.06 kJ;5;CHEM 1151 General Chemistry for Engineers;Fall 2011;Section B: Open-response questions (10 pts each);Show your work to receive credit;15. Copper (Cu) crystallizes in a face-centered cubic unit cell. If the radius of an atom of copper;is 128 pm, what is the density (in g/cm3) of copper?;6;CHEM 1151 General Chemistry for Engineers;Fall 2011;16. Consider the following two vessels containing pure gases;Vessel 1: 1.50 L of He(g) at 250. K & 2.50 atm;Vessel 2: 1.00 L of O2(g) at 350. K & 1.50 atm;The contents of these two vessels are mixed at 300. K in a third vessel having a volume of;2.00 L.;a. Determine the partial pressure of O2 (in atm) in the third vessel.;b. Determine the concentration of O2 (in M) dissolved in water in contact with the gas in the;third vessel if the Henrys Law constant for O2 in water is 1.3010-3 M/atm.;7;CHEM 1151 General Chemistry for Engineers;17. Consider the following reaction;CaCO3(s) + 2 HCl(aq) CaCl2(aq) + H2O(l) + CO2(g);We react 100. g of calcium carbonate with 100. g of hydrochloric acid.;a. Determine the limiting reactant.;b. What is the mass (in g) of water produced?;8


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