Docsity
Log inSign up
Docsity
Prepare for your exams
Prepare for your exams

Study with the several resources on Docsity

Earn points to download
Earn points to download

Earn points by helping other students or get them with a premium plan

Guidelines and tips
Guidelines and tips
Sell on Docsity
Sell on Docsity
Log inSign up

Prepare for your exams

Study with the several resources on Docsity

Find documents

Prepare for your exams with the study notes shared by other students like you on Docsity

Search Store documents

The best documents sold by students who completed their studies

Search through all study resources
Docsity AINEW

Summarize your documents, ask them questions, convert them into quizzes and concept maps

Explore questions

Clear up your doubts by reading the answers to questions asked by your fellow students

Earn points to download

Earn points by helping other students or get them with a premium plan

Share documents
download point icon20 Points

For each uploaded document

Answer questions
download point icon5 Points

For each given answer (max 1 per day)

All the ways to get free points
Get points immediately

Choose a premium plan with all the points you need

Study Opportunities

Choose your next study program

Get in touch with the best universities in the world. Search through thousands of universities and official partners

Community

Ask the community

Ask the community for help and clear up your study doubts

University Rankings

Discover the best universities in your country according to Docsity users

Free resources

Our save-the-student-ebooks!

Download our free guides on studying techniques, anxiety management strategies, and thesis advice from Docsity tutors

From our blog

Exams and Study
Go to the blog

Exam 1, Version A for General Chemistry II | CHEM 113, Exams of Chemistry

Colorado State University (CSU)Chemistry

Material Type: Exam; Class: General Chemistry II; Subject: Chemistry; University: Colorado State University; Term: Fall 2016;

Typology: Exams

2015/2016
On special offer
30 Points
Discount

Limited-time offer

Uploaded on 10/04/2016

unknown user
unknown user 🇺🇸

5

(2)

2 documents

1 / 9

Toggle sidebar

This page cannot be seen from the preview

Don't miss anything!

bg1
Department of Chemistry
CHEM 113 – Exam
1
–
Version A
September 14, 2016
Name
(printed):
*Please, read the instructions and make sure you understand them*
For this exam, you will need a pencil, a TI-30Xa (or solar) or a TI-30X IIS calculator (without
the cover), and your CSU ID card. NO OTHER MATERIALS are allowed on your desk
during the exam. Calculators may not be shared.
When you have finished taking the exam, both the cover sheet and the answer sheet must be
turned in. Make sure to bubble in your CSU ID number and version letter on your answer sheet.
You will be graded solely on the answers that you report on your answer sheet, so be sure to
bubble your exam version and answers in carefully. You will not be granted extra time to transfer
your answers from your exam booklet to your answer sheet, so plan your time accordingly.
Use of CELL PHONES or smartwatches for any purpose during the exam will be
considered unauthorized assistance and any violators will be referred to the Student
Resolution Center.
Sign your answer sheet to affirm the CSU honor pledge.
***When you have finished taking the exam, the answer sheet and cover sheet must be turned in.***
This exam has a total of 25 questions for a total of 5 pages (9 printed sides/pages) including this
page and page 2, which contains constants, equations, a periodic table, and other potentially
useful data. All questions are equally weighted at 5 points each. *Choose the one best answer
to each question* Try to relax and do your best!
pf3
pf4
pf5
pf8
pf9
Discount

On special offer

Partial preview of the text

Download Exam 1, Version A for General Chemistry II | CHEM 113 and more Exams Chemistry in PDF only on Docsity!

Department of Chemistry

CHEM 113 – Exam 1 – Version A

September 14, 2016

Name (printed):

*Please, read the instructions and make sure you understand them *

For this exam, you will need a pencil, a TI- 30 Xa (or solar) or a TI-30X IIS calculator (without the cover), and your CSU ID card. NO OTHER MATERIALS are allowed on your desk during the exam. Calculators may not be shared. When you have finished taking the exam, both the cover sheet and the answer sheet must be turned in. Make sure to bubble in your CSU ID number and version letter on your answer sheet. You will be graded solely on the answers that you report on your answer sheet, so be sure to bubble your exam version and answers in carefully. You will not be granted extra time to transfer your answers from your exam booklet to your answer sheet, so plan your time accordingly. Use of CELL PHONES or smartwatches for any purpose during the exam will be considered unauthorized assistance and any violators will be referred to the Student Resolution Center.

Sign your answer sheet to affirm the CSU honor pledge.

When you have finished taking the exam, the answer sheet and cover sheet must be turned in. This exam has a total of 25 questions for a total of 5 pages ( 9 printed sides/pages) including this page and page 2, which contains constants, equations, a periodic table, and other potentially useful data. All questions are equally weighted at 5 points each. Choose the one best answer to each question Try to relax and do your best!

Potentially useful equations: 𝑆 = 𝑘𝐵 ln 𝑊 , 𝑘𝐵 = 1. 38 × 10 −^23 𝐾𝐽 ∆𝑆𝑢𝑛𝑖𝑣 = ∆𝑆𝑠𝑦𝑠 + ∆𝑆𝑠𝑢𝑟𝑟 ∆𝐻𝑟𝑥𝑛^ °^ = ∑ 𝑚∆𝐻𝑓^ °^ ,𝑝𝑟𝑜𝑑𝑢𝑐𝑡𝑠− ∑ 𝑛∆𝐻𝑓^ °,^ 𝑟𝑒𝑎𝑐𝑡𝑎𝑛𝑡𝑠 ∆𝐺𝑟𝑥𝑛^ °^ = ∆𝐻𝑟𝑥𝑛^ °^ − 𝑇∆𝑆𝑟𝑥𝑛^ ° ∆𝐺𝑟𝑥𝑛^ °^ = ∑^ 𝑚∆𝐺𝑓^ °^ ,𝑝𝑟𝑜𝑑𝑢𝑐𝑡𝑠− ∑^ 𝑛∆𝐺𝑓^ °^ ,𝑟𝑒𝑎𝑐𝑡𝑎𝑛𝑡𝑠 ∆𝑆𝑠𝑢𝑟𝑟 = − ∆𝐻𝑠𝑦𝑠 𝑇 ∆𝑆𝑟𝑥𝑛^ °^ = ∑ 𝑚𝑆𝑓^ °,^ 𝑝𝑟𝑜𝑑𝑢𝑐𝑡𝑠− ∑ 𝑛𝑆𝑓^ °,^ 𝑟𝑒𝑎𝑐𝑡𝑎𝑛𝑡𝑠 T(K) = T(°C) + 273. 1A (^) PERIODIC TABLE OF THE ELEMENTS 8A 1 H 1.008 2A 3A 4A 5A 6A 7A 2 He

3 Li

4 Be

5 B

6 C

7 N

8 O

9 F

10 Ne

11 Na

12 Mg 24.31 3B 4B 5B 6B 7B 8B 8B 8B 1B 2B 13 Al

14 Si

15 P

16 S

17 Cl

18 Ar

19 K

20 Ca

21 Sc

22 Ti

23 V

24 Cr

25 Mn

26 Fe

27 Co

28 Ni

29 Cu

30 Zn

31 Ga

32 Ge

33 As

34 Se

35 Br

36 Kr

37 Rb

38 Sr

39 Y

40 Zr

41 Nb

42 Mo

43 Tc (98) 44 Ru

45 Rh

46 Pd

47 Ag

48 Cd

49 In

50 Sn

51 Sb

52 Te

53 I

54 Xe

55 Cs

56 Ba

57 La

72 Hf

73 Ta

74 W

75 Re

76 Os

77 Ir

78 Pt

79 Au

80 Hg

81 Tl

82 Pb

83 Bi

84 Po (209) 85 At (210) 86 Rn (222) 87 Fr (223) 88 Ra (226) 89 Ac ( 227 ) 104 Rf ( 265 ) 105 Db ( 268 ) 106 Sg ( 271 ) 107 Bh ( 270 ) 108 Hs ( 277 ) 109 Mt ( 276 ) 110 Ds ( 281 ) 111 Rg ( 280 ) 112 Cn (285) 114 Fl ( 289 ) 116 Lv ( 293 )

  1. The _____ Law of Thermodynamics states that the entropy change in an isolated system during a spontaneous process must be greater than zero: A. Zeroth B. First C. Second D. Third E. None is correct.
  2. At 0 K, the entropy of a perfect crystal is: A. > 0 B. = 0 C. < 0 D. > 0 or < 0, depending on the chemical structure of the crystal. E. ≥ 0, depending on the chemical structure of the crystal.
  3. During which of the following processes is ΔS°sys < 0? A. Salt crystals dissolve in water. B. Air escapes from a hole in a balloon. C. Elemental iron and oxygen react to form rust (Fe 2 O 3 ). D. Ice melts in your hand. E. Water boils in a pan.
  4. Calculate ΔS°rxn for the reaction below. The molar standard entropy (S°) for each species can be found in Table 12.2 on the cover sheet. 2CH 3 CH 3 (g) + 7O 2 (g) → 4CO 2 (g) + 6H 2 O(g) A. – 94.0 J/K B. +550.9 J/K C. +94.0 J/K D. +337.1 J/K E. – 550.9 J/K
  5. Consider the following three changes in the possible distribution of six gaseous particles within three interconnected boxes. Which change has a ΔS > 0? A. I only B. II only C. III only D. I and II E. II and III
  1. Which of the following substances would you expect to have the highest entropy at the same temperature? A B C D E
  2. The standard free energy, ΔGo, of different processes is listed below. What of these processes is spontaneous? I. H 2 O( g ) + C( s ) → H 2 ( g ) + CO( g ); ΔGo^ = +91 kJ at 298K II. NH 4 NO 3 (s) → NH 4 +(aq) + NO 3 - (aq); ΔGo^ = – 4.4 kJ at 298K III. N 2 (g) + 3H 2 (g) → 2NH 3 (g); ΔGo^ = +61.44 kJ at 773K A. Reaction I only B. Reaction II only C. Reaction III only D. Reactions I and II E. Reaction I and III
  3. Which of the following is always true for a spontaneous exothermic process? A. Δ Ssys < 0 B. Δ Ssurr > 0 C. Δ Suniverse = 0 D. Δ Ssys > 0 E. Δ Ssurr < 0
  4. What is the entropy change in the surroundings, Δ S surr, when 1.50g of ice melts at 0.00°C in a large room maintained at 32.0°C? The heat of fusion, Δ H fus, of ice is +6.01 kJ/mol. A. +22.0 J/K B. +1.64 J/K C. – 22.0 J/K D. +188 J/K E. – 1.64 J/K
  1. Why does the conversion of the ATP to ADP (Reaction 1) often occur simultaneously with other biochemical reactions such as the production of sucrose shown in Reaction 2? ΔG Reaction 1: ATP → ADP + H 2 PO 4 – 30 kJ/mol Reaction 2: glucose + fructose → sucrose +27 kJ/mol A. Reaction 1 is exothermic, so it can provide the heat energy to fuel endothermic reactions, such as Reaction 2. B. Entropy increases in Reaction 1 but decreases in Reaction 2. Reactions where entropy decreases cannot happen without being coupled to a reaction where entropy increases. C. The product of Reaction 1, ADP, is a reactant in the production of sucrose shown in Reaction 2. D. Reaction 1 is a spontaneous reaction in which free energy is released. This released free energy can be used as the driving force for a nonspontaneous reaction, such as Reaction 2. E. The conversion of ATP to ADP (Reaction 1) cannot happen alone because it requires the input of work, which can be provided from the free energy change in Reaction 2.
  2. What are the signs of ΔS, ΔH, and ΔG for the condensation of water on the sides of a glass of ice tea at room temperature? A. +, +, – B. – , +, – C. +, – , – D. – , +, + E. – , – , –
  3. The synthesis of ammonia is shown below. Under standard conditions, ΔHo^ = – 92.2 kJ and ΔS = – 198.3 J/K for this reaction. Which of the following best describes the spontaneity of this reaction at 25oC? N 2 (g) + 3 H 2 (g) → 2 NH 3 (g) A. The reaction is spontaneous at all temperatures (including 25oC) because both enthalpy and entropy decrease in the reaction. B. The reaction is spontaneous at 25oC because free energy decreases at this temperature. C. The reaction is nonspontaneous at 25 oC because free energy increases at this temperature. D. The reaction is neither spontaneous nor nonspontaneous at 25oC because it is at equilibrium. E. The spontaneity of this reaction cannot be determined without the free energies of formation for the reactants and products.
  1. Consider the sublimation of iodine shown below. If ΔSo^ = +144.6 J/K and ΔHo^ = +62.4 kJ for the reaction, what is the sublimation point (the temperature at which sublimation occurs) for iodine in Kelvin? I 2 (s) → I 2 (g) A. 0.432 K B. 2.32 K C. 432 K D. 2320 K E. 82.2 K
  2. Which of the following does not accurately describe reaction rates? A. Rates of reactions generally decrease over the course of the reaction. B. Overall rate of a reaction is always positive and has units of concentration over time. C. The average rate of a reaction represents the relative change in concentration of a reactant or product over a specific time period. D. The instantaneous rate of a reaction is a more accurate description of the actual rate of a reaction than the average rate of a reaction at a given point in time. E. The instantaneous rate of a reaction represents the initial rate of a reaction (at t = 0.)
  3. Concentration data for the reaction below are shown in the table. Use this data to determine the average rate of the reaction below from t = 10.0 s to t = 20.0 s. 2 A → 2 B A. 0.04 M/s B. 1.4 M/s C. 7. M/s D. 0.4 M/s E. 0.7 M/s Time (s) [A] (M) [B] (M) 0.0 4.1 0. 5.0 3.1 1. 10.0 2.5 1. 15.0 2.1 2. 20.0 1.8 2. 30.0 1.4 2.