CHE 132 Spring 2022 Final Exam Version A

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Stony Brook University *

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132

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Chemistry

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Jan 9, 2024

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pdf

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Uploaded by ProfessorParrotMaster176 on coursehero.com

CHE 132 Final Exam Form 1A Spring 2022 Directions 1. Place all other items besides your exam out of sight and or beneath your seat. 2. Place your ID (face up), pencils, erasers, and a scientific calculator at your desk now. You may be asked to show proof of ID and sign an attendance sheet. 3. On your scantron, starting from the left, write and bubble – in your (leave extra spaces blank):  SBID NUMBER under IDENTIFICATION NUMBER 4. Print your name clearly and sign. 5. DO NOT OPEN YOUR EXAM until told to do so. 6. All scantron forms must be submitted after 150 minutes. No extra time will be given. 7. All answers must be entered on the Scantron answer sheet, which you must turn in. 8. Answer sheets will not be returned, so record your answers next to each question on the exam for comparison with the answers when they are posted on Blackboard. Use the space between questions, the backs of pages, or the extra sheets for analysis and calculations. 9. There are 40 questions on this exam and 8 total pages. 10. For multiple choice questions, bubble in the letter of the one choice that best completes the statement or answers the question on the scantron form. No credit will be given for multiple answers. 11. Short Answer/Numerical – Check to make sure that you • skip the multiple – choice scantron # when you have a short answer. • e nter your answers on the right – hand side of the scantron in the appropriately numbered line . • Work will not be graded or afforded partial credit. 12. Once you open the exam, be sure you have all the pages including a Periodic Table and a sheet of equations/conversion factors. General Chemistry Policies:  Possession of cell phones, smart watches, other communication devices, or any unauthorized materials during the exam will result in a grade of 0 on this exam, a report to Academic Judiciary, and a possible grade of F for the course.  If you do not have an ID, note that on the sign – in sheet, and you must see Dr. Amarante the day after the exam and show her a valid ID.

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CHE 132 Final Exam Equations D H soln = -E lattice + D H hydration K = ° C + 273.15 ° F = 9/5 ( ° C) + 32 d=m/V M 1 •V 1 =M 2 •V 2 ∆࠵? = ࠵? + ࠵? ∆࠵? = ࠵? ! ࠵? = ࠵?࠵? "! ∆࠵? ∆࠵? #$% ° = ∑ ࠵? ∆࠵? ’ ° (࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?) − ∑ ࠵? ∆࠵? ’ ° (࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?) ࠵? = ࠵? ( ࠵?࠵?࠵? ∆࠵? = ) !"# * ∆࠵? "+## = − ∆- * ∆࠵? .#/%" = ∆- $!%&’ * $!%&’ ∆࠵? +%01 = ∆࠵? "2" + ∆࠵? "+## ∆࠵? #$% ° = ∑ ࠵? ࠵? ° (࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?) − ∑ ࠵? ࠵? ° (࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?) D G = D H-T D S ∆࠵? #$% ° = ∑ ࠵? ∆࠵? ’ ° (࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?) − ∑ ࠵? ∆࠵? ’ ° (࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?) Rate=k[A] m [B] n ࠵? 3/5 = 3 6[8] ( ࠵? 3/5 = [8] ( 56 ࠵? 3/5 = :.<=> 6 ln[࠵?] . = −࠵?࠵? + ln[࠵?] : 3 [8] $ = ࠵?࠵? + 3 [8] ( [ ࠵?] . = −࠵?࠵? + [࠵?] : [࠵?] . = [࠵?] : ࠵? ?6. ࠵? = ࠵?࠵? ? ) % *+ ࠵?࠵? 6 , 6 - = − @ % A E 3 * , − 3 * - F ln ࠵? = − @ % A 3 * + ln ࠵? ࠵?࠵? ! = − log ࠵? ! ࠵?࠵? = − log[࠵? " ࠵? # ] ࠵?࠵? = ࠵?࠵? $ + ࠵?࠵?࠵? [& — ] [(&] ࠵?࠵?࠵? = ࠵?࠵? ! + ࠵?࠵?࠵? [)( " ] [)] %࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵? = [( # * " ] $% [(&] &’&(&)* ࠵? 100% ∆࠵?° = −࠵?࠵?࠵?࠵?࠵? ∆࠵?° = −࠵?࠵?࠵? +,-- ° ࠵? +,-- ° = /0 12 ࠵?࠵?࠵? ࠵? +,-- = ࠵? +,-- ° — /0 12 ࠵?࠵?࠵? ࠵? +,-- ° = ࠵? +$3456, ° − ࠵? $156, ° or ࠵? +,-- ° = ࠵? 7,68+3951 ° + ࠵? 5:96$3951 ° ࠵? +,-- ° = ;.;=>?@ 1 ࠵?࠵?࠵?࠵? ࠵?࠵? 298.15 ࠵? ࠵? +,-- = ࠵? +,-- ° — ;.;=>? @ 1 Units Conversions 1 m = 1.0936 yds 1 cm = 0.39370 inch 760 torr = 1 atm 1 inch = 2.54 cm 1 km = 0.621371 mile 760 mm Hg = 1 atm 1 Å = 10 -10 m 1 mL = 1 cm 3 101,325 Pa = 1 atm 1 kg = 2.2046 lbs 1 L = 10 -3 m 3 1.013 bar = 1 atm 1 lb = 453.59 g 1 gallon = 3.7854 L 1 Pa = 1 N/m 2 1 lb = 16 oz 1 quart = 0.94633 L 4.184 J = 1 cal 1 ton = 2000 lbs 1 mol = 6.022 X 10 23 4 qts = 1 gallon C = k H P P solution = χ solvent P solvent o Δ T = K b m solute Δ T = K f m solute Π = MRT Δ T = iK f m solute Π = iMRT Δ T = iK b m solute K c = [ C ] c [ D ] d [ A ] a [ B ] b K p = p C c p D d p A a p B b K p = K c ( RT ) Δ n a x = x ⎡ ⎣ ⎤ ⎦ ° c a i = p i p ref x = − b ± b 2 − 4 ac 2 a K w = [H 3 O + ][OH — ] =[H + ][OH — ]= 1.0 x 10 -14 at 25 °C K a xK b = K w pK a = − log K a pOH = − log[ OH − ] pH + pOH = 14.00 = pK w ࠵?࠵?࠵?࠵? at 298.15 K

Table 1. K a and K b values for common acids and bases at 25.0°C. Table 2. Physical properties and constants for solvents. Solvent Boiling Point (°C) K b (°C/m) Freezing Point (°C) K f (°C/m) Water 100.0 0.512 0.0 1.86 Ethanol 78.2 1.22 -114.1 12.5 Aniline 184.3 3.69 -5.96 5.87 Table 3. Henry’s Law constants for select gases at 25.0 °C. Gas k H (M/atm) O 2 1.3 x 10 -3 N 2 6.1 x 10 -4 CO 2 3.4 x 10 -2 NH 3 5.8 x 10 1 Name K a Name K b H 2 C 2 O 4 (Ka 1 ) 5.9 x 10 -2 Ethylamine (CH 3 CH 2 NH 2 ) 4.3 x 10 -4 HSO 4 – 1.2 x 10 -2 Methylamine (CH 3 NH 2 ) 4.4 x 10 -4 H 2 SO 3 (Ka 1 ) 1.2 x 10 -2 Dimethylamine [(CH 3 ) 2 NH] 5.9 x 10 -4 Chlorous acid (HClO 2 ) 1.1 x 10 -2 Diethylamine [(CH 3 CH 2 ) 2 NH] 8.6 x 10 -4 Citric acid (H 3 C 6 H 5 O 7 , Ka 1 ) 7.4 x 10 -3 Trimethylamine [(CH 3 ) 3 N] 7.4 x 10 -5 H 3 PO 4 (Ka 1 ) 7.2 x 10 -3 Ammonia (NH 3 ) 1.76 x 10 -5 Hydrofluoric acid (HF) 6.8 x 10 -4 Pyridine (C 5 H 5 N) 1.7 x 10 -9 Nitrous acid (HNO 2 ) 4.6 x 10 -4 Hydroxylamine (NH 2 OH) 6.6 x 10 -9 Cyanic acid (HCNO) 3.5 x 10 -4 Aniline (C 6 H 5 NH 2 ) 4.0 x 10 -10 Formic acid (HCOO H ) 1.8 x 10 -4 Lactic acid 1.4 x 10 -4 HC 2 O 4 – 6.4 x 10 -5 Benzoic acid (C 6 H 5 COO H ) 6.3 x 10 -5 Hydrazoic acid (HN 3 ) 1.9 x 10 -5 Acetic acid (CH 3 COO H ) 1.8 x 10 -5 Propanoic acid (CH 3 CH 2 COO H ) 1.3 x 10 -5 H 2 CO 3 (Ka 1 ) 4.2 x 10 -7 H 2 PO 4 – (Ka 2 ) 6.3 x 10 -8 HSO 3 – 6.2 x 10 -8 HClO 2.9 x 10 -8 HBrO 2.3 x 10 -9 HCO 3 — (Ka 2 ) 4.8 x 10 -11 HPO 4 2— (Ka 3 ) 4.2 x 10 -13

Table 4 . Solubility Product Constants at 25 °C.

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