This preview shows page 1. Sign up to view the full content.
Unformatted text preview: Chemistry 1A Fall 2000
__________________________________________________________________________________ Final Exam, Version A
December 13, 2000
(Closed book, 180 minutes, 350 points) Name: ______________________ Section Number: ____________________ SID: _______________________ T.A. Name: ________________________ Exam information, extra directions, and useful hints to maximize your score:
• Write your name on all fourteen pages. • There are two parts to the exam: 1) multiple choice and 2) short answer problems. • For the multiple choice problems, fill in the ScantronTM form AND circle the answer on your exam. • Answer the questions you know how to do first, then work on the questions you skipped. • Show all work on the short answer problems for which you want credit and do not forget to include units! • You may use the back side of the exam pages for scratch paper. • Some possibly useful equations and diagrams are given on Page 2. (Do not write in this box; it is for official use only.)
Page Points 3-10
Total / 175
/ 350 Page 2 of 2 Name:_________________________________________ Useful information:
milli, m (x 10-3) micro, ì (x 10-6) nano, n (x 10-9)
kilo, k (x 103)
mega, M (x106) giga, G (x 109) Ekin (e-) = hí – Ö = hí - hío = mv2/2
En = − 2 R ∞
n Ephoton = hí = hc/ë
ë de Broglie= h/p = h/mv 3
∆G = ∆H - T∆S
∆E = q + w
∆G = ∆Go + RTlnQ
pX = - log [X]
pH = pKa + log [A-]/[HA] PV= nRT
q = m Cp°∆T
Cp°(H2O, λ)= 1 cal/K•g = 4.184 J/K•g
S = kBlnW
∆Go = - RTlnK
ln K = -∆Ho/RT + ∆So/R ∆H o = ∑ ∆H o (products) − ∑ ∆H o (reactants)
f Bond H-H
O=O ∆S = ∑ S (products) − ∑ S (reactants)
o o o ∆G o = ∑ ∆G o (products) − ∑ ∆G o (reactants)
f Average Bond Enthalpy (kJ/mol) 436
497 Compound ∆ Hf° (kJ/mol) at 25oC S° (J/mol-K) at
25oC ∆ Gf° (kJ/mol)
at 25oC NH4NO3 (s)
-108.7 Ksp(AgCl) = 1.8 x 10-10 Page 3 of 3 Name:_________________________________________ Part 1: Multiple Choice.
(5 pts each, 175 pts total)
Instructions: Bubble in the correct answer on your Scantron sheet AND circle the answer on your exam.
Each question has one correct answer.
1.) The answer to question 1 is A. Bubble in A on your Scantron™ form. 2.) Which of the following has the highest NO bond order?
− A.) NO 3.) + C.) NO2 − D) NO2 + E.) NO3 − In order that the diagram below correctly depict the structure of ICl2−, at what positions should the
Cl atoms be drawn? A.) 1,2 4.) B.) NO B.) 1,4 C.) 2,3 D.) 2,5 E.) 4,5 A compound contains carbon, hydrogen, and oxygen in the mass percentages given below. What
is its empirical formula?
A.) CHO B.) CH2O H: 6.7% C.) C2H6O O: 53.3% D.) C3H6O E.) C3H6O2 Page 4 of 4
5.) Two moles of an element are added to a vessel of volume approximately 20 L containing oxygen
gas at a pressure of 2 atm at 0°C. All of the element reacts, yielding 1 mole of an oxide and ½ atm
of oxygen gas. Which of the following could be the oxide?
A.) Na2O 6.) CO2 D.) Al2O3 E.) P4O10 B.) Orange C.) Yellow D.) Green E.) Violet B.) C2H3Cl C.) C2H2Cl2 D.) C2HCl3 E.) C2Cl4 Which transition in He+ has the same energy difference as the n = 1 à n = 2 transition in a
A.) 1 à 2 9.) C.) Which of the following compounds from among ethylene (H2C=CH2) and its chlorinated
derivatives has the greatest number of structural isomers?
A.) C2H4 8.) B.) CaO Blue light (450 nm) ejects photoelectrons from potassium (K) atoms. Light of which color could
eject photoelectrons with the same kinetic energy from magnesium (Mg) atoms?
A.) Red 7.) Name:_________________________________________ B.) 1 à 3 C.) 2à 3 D.) 2 à 4 E.) 3 à 4 Which of the following species has the highest ionization energy?
A.) H (1s) B.) H (2s) C.) He+ (2s) D.) He (1s2) E.) He (1s2p) Page 5 of 5 10.) Which of the following does not correspond to an allowed orbital (set of quantum
A.) 1s 11.) C.) 3d D.) 4f E.) 5f B.) P C.) Mg D.) Si E.) Na Which of the following atoms or ions is paramagnetic in its ground state?
A.) Be 13.) B.) 2d Identify X from the electronic configuration of the ion X− (1s22s22p63s2).
A.) Al 12.) Name:_________________________________________ − B.) Cl C.) Ar D.) O E.) Zn D) Cl E) S Which has the smallest atomic radius?
A) Ca B) K C) Ar Page 6 of 6 14.) Name:_________________________________________ Select the figure with the correct molecular orbital diagram and bond order. A.) B.) C.) D.) 15.) At a constant pressure of 3.00 atm, 2.00 L of air is cooled from 10.0 °C to –75.0 °C.
What is the new volume?
A.) 0.27 L 16.) E.) B.) 1.40 L C.) 2.96 L D.) 6.14 L E.) 13.0 L The root-mean-square speed of 16O16O is 482 ms-1 at STP. What is the rms speed of
O O at STP?
A.) 441 ms-1 B.) 461 ms-1 C.) 482 ms-1 D.) 501 ms-1 E.) 527 ms-1 Page 7 of 7 17.) Name:_________________________________________ The equilibrium constant for the endothermic reaction
N2O4 (g) 2NO2 (g) at 25° C is K = 8.8. Which could be the magnitude of the equilibrium constant K at 34° C?
A) 1.1 18.) B) 2.2 C) 4.4 D) 8.8 E) 17.6 For the following reaction at 25° C,
CH2ClCOO- (aq) + H3O+ (aq) CH2ClOOH (aq) + H2O (l) the equilibrium concentrations are [CH2ClCOOH]=0.0888 M, [CH2ClCOO-]=[H3O+]=0.0112 M,
and [H2O]=55 M. What is the magnitude of the equilibrium constant K?
A.)2.57 x 10-5 19.) C.) 1.4 x 10-3 D.) 8.88 x 10-2 E.) 1.26 x 10-1 Air contains approximately 20 mole percent oxygen and 80 mole percent nitrogen. How many
millimoles of molecular oxygen (Henry’s Law constant: K=1.3 mM/atm) are dissolved in a glass
of water (~200mL) at atmospheric pressure?
A.) 32.5 20.) B.) 1.25 x 10-4 B.) 6.5 C.) 1.3 D.) 0.26 E.) 0.052 For the reaction
CaO (s) + CO2 (g) CaCO3 (s) ∆H°~ -200 kJ/mol and ∆S°~ -200 J/K•mol. At which temperatures is the reaction spontaneous at
1atm? A.) above 1000 K B.) below 1000 K C.) only at 1000 K D.) at all T E.) at no T Page 8 of 8 21.) Name:_________________________________________ Consider the gas phase equilibrium reaction:
A(g) B(g) + C(g). You decide to carry out this reaction in your flask. The equilibrium constant for this reaction is
K and the reaction is known to be endothermic. Assume that you start with only gas A in your
flask and you let the system come to equilibrium. Now, you place your flask in the refrigerator
(i.e. you suddenly lower the temperature). In which direction will the reaction proceed? A.)
E.) 22.) Right. Q is now less than K.
Right. Q is now greater than K.
No change. The system is already at equilibrium and Q is equal to K.
Left. Q is now less than K.
Left. Q is now greater than K. The following figure shows the temperature dependence of the equilibrium constant, K, for
the equilibrium between the liquid and gas phases of an unknown alcohol. Alcohol (l) Alcohol (g) What temperature is the normal boiling point of the alcohol (i.e. at sea level)?
A.) 0 °C B.) 20 °C C.) 40 °C D.) 60 °C E.) >60 °C Page 9 of 9
23.) 1.0 mole of ammonium nitrate (NH4NO3) is dissolved in 1.0 liter of water at 25
data provided on Page 2, determine the final temperature of the solution.
A.) -6.7 24.) Name:_________________________________________ C B.) 6.7 C C.) 18.3 C D.) 28.0 C The acid ionization constants are Ka1 for NH4+ and Ka2 for HAc. What is K for the following
Ac− (aq) + NH4+ (aq) HAc (aq) + NH3 (aq)
A.) Kw 25.) C E.) 31.7 C. Using the B.) Ka1 Ka2 C.) ( Ka1 Ka2 ) / Kw D.) Ka1 / Ka2 E.) Ka2/ Ka1 You dissolve 0.10 moles of an unknown acid in water and the resulting solution has a volume of
1.0 L. You measure the concentration of H3O+ in this solution and the pH is 3.0. Which of the
following statements is true for this unknown acid?
A.) It is a strong acid because the relative Gibbs free energy of the products is higher than that of
B.) It is a strong acid because the relative Gibbs free energy of the products is lower than that
of the reactants. C.) It is a weak acid because the relative Gibbs free energy of the products is higher than that
of the reactants. D.) It is a weak acid because the relative Gibbs free energy of the products is lower than that of
E.) 26.) It is a weak acid because the relative Gibbs free energy of the products equals that of
the reactants. A sample of formic acid (HA, a weak acid) is titrated to the equivalence point with 50 mL of 0.1
M NaOH. 25 mL of 0.1 M HCl are then added to the solution. What is the value of the ratio
A.) 0 B. ) 0.5 C. ) 1 D. ) 2 E. ) ∞ Page 10 of 10 27.) Name:_________________________________________ For the amino acid glycine the carboxyl group (COOH) has a pKa = 2.0 and the amino
group (NH3+) has a pKa = 9.0. Which is the dominant form of glycine in a solution with
pH = 6.0?
- A.) H2NCH2COOH
E.) H3NCH2C(OH)2+ For each of the following questions, choose the sketch which best represents the indicated
relationship. 2AlBr3(s). 28.) ln K vs. 1/T for 2Al(s) + 3Br2(g) 29.) ∆Gº vs. T for the reaction in Question 28. 30.) PNO2 vs. PN2O4 at constant T for N2O4 (g) 31.) [Ag+ (aq)] vs. [Cl (aq)] for a solution of 0.1M AgNO3 titrated with HCl. 32.) Photon energy vs. wavelength (ë) for electromagnetic radiation. 33.) UV absorbance vs. concentration of diluted sun screen lotion 34.) ∆T vs. mass of a metal for a given heat q. 35.) Kinetic energy vs. T for an ideal gas. 2NO2 (g). − Page 11 of 11 Name:_________________________________________ Part 2: Short Answer Problems (175 pts total)
Instructions: Enter answers in the boxes provided. Show your work. Where requested
write explanations in fifteen words or less.
1.) (52 points)
There is strong evidence that chlorofluorocarbons (CFCs) are responsible for the “ozone hole”
which has occurred in the stratosphere over the South Pole. The ClO radical is involved in this
ozone destruction cycle. It is highly reactive and has a tendency to react with ozone (O3) and
a.) The Lewis structure of the ClO radical is given below. Sketch the Lewis structures for the
ClO+ and ClO ions.
− + ClO Structure: ClO Structure:
+ b.) __ Considering the information on Page 2, would you expect a ClO radical to react with an O
atom in the stratosphere to form an O2 molecule and a chlorine atom. Circle your choice
YES NO Not enough information Explanation: c.) Using the data on Page 2, estimate the enthalpy change for the relevant reaction: Cl(g) + O2(g). ClO(g) + O(g)
Cl-O bond enthalpy = 270 kJ/mol d.) ÄHo: O=O bond enthalpy = 497 kJ/mol ClO radicals in the stratosphere are formed from the reaction of Cl atoms with O3. The Cl
atoms in turn are generated when sunlight hits CFCs like CF2Cl2 (also known as Freon-12).
Calculate the maximum wavelength (in nanometers) required to break a C-Cl bond in
CF2Cl2 using the data on Page 2.
C-Cl bond enthalpy = 389 kJ/mol
Ephoton = hc/ë ëmax: Page 12 of 12
2.) Name:_________________________________________ (75 points)
Consider the following five solutions in the titration of the weak acid formic acid (HA)
with a strong base at 25oC. For this problem, explicitly calculate all quantities. T itration Curve for Formic Acid (HA)
9 .0 p H 7 .0
0 .0 5 0.0 1 00.0 1 50.0 2 00.0 m l 0.10 M NaOH solution
a dded a.) Calculate the pH of a 100 mL solution of 0.100 M formic acid (HA, pKa = 3.75)?
pH: b.) To a 100 mL solution of 0.100 M HA, 20 mL of 0.100 M NaOH are added.
Calculate the pH of this solution.
pH : Page 13 of 13
c.) Name:_________________________________________ To a 100 mL solution of 0.100 M HA, 100 mL of 0.100 M NaOH are added.
Calculate the pH of this solution.
pH: d.) To a 100 mL solution of 0.100 M HA, 160 mL of 0.100 M NaOH are added.
Calculate the pH of this solution.
pH: e.) To a 100 mL solution of 0.100 M HA, 100 mL of 0.100 M NaOH and 40 mL of
0.100 M HCl are added. Calculate the pH of this solution.
pH: Page 14 of 14
3.) (2 pts each, 48 pts total) Name:_________________________________________ A gas first expands isothermally against a vacuum (process I) and then is compressed
isothermally and reversibly to its original volume and temperature (process II).
Determine the value (0, < 0, > 0) for each of the quantities below for process I, process II,
and the overall cyclic process (I+II), and circle your choice. Each of the 24 boxes should
have one choice circled. I
Q II I+II >0 0 <0 >0 0 <0 >0 0 <0 >0 0 <0 ∆Esys >0 0 <0 >0 0 ∆Esurr >0 0 <0 >0 ∆Euniv >0 0 <0 ∆Ssys >0 0 ∆Ssurr >0 ∆Suniv. >0 W >0 0 <0 >0 0 <0 <0 >0 0 <0 0 <0 >0 0 <0 >0 0 <0 >0 0 <0 <0 >0 0 <0 >0 0 <0 0 <0 >0 0 <0 >0 0 <0 0 <0 >0 0 <0 >0 0 <0 ...
View Full Document
This note was uploaded on 03/30/2010 for the course CHEM 1A taught by Professor Nitsche during the Spring '08 term at University of California, Berkeley.
- Spring '08