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## Practice Notes

1 review
by: Maura Lynch-Miller

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# Practice Notes

Marketplace > University of Chicago > > Practice Notes
Maura Lynch-Miller
UChicago
GPA 4.0

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Practice Notes
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"If you want to pass this class, use these notes. Period. I for sure will!"
Kaela

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This 2 page Class Notes was uploaded by Maura Lynch-Miller on Wednesday January 13, 2016. The Class Notes belongs to at University of Chicago taught by in Winter 2016. Since its upload, it has received 57 views.

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## Reviews for Practice Notes

If you want to pass this class, use these notes. Period. I for sure will!

-Kaela

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Date Created: 01/13/16
Problem Set 5A 1. Problem 4.88 + some: Balance each of the following oxidation-reduction reactions. Indicate the oxidation number of each atom, the oxidizing agent, the reducing agent, the species being oxidized and the species being reduced. For (a) and (c), write each half-reaction. 3+ - a. Cl (2) + Al(s) --> Al (aq) + Cl(aq) b. O (2) + H O(2) + Pb(s)  Pb(OH) 2 + - 2+ 2+ 3+ c. H (aq) + MnO (aq) 4 Fe (aq)  Mn (aq) + Fe (aq) + H O(l) 2 2. Parts of Problem 4.80/82: Assign oxidation numbers to all of the atoms in each of the following: a. UO 2+ 2 b. As O 2 3 c. NaBiO 3 d. (NH )4 2(SO ) 4 3 3. Part of 18.30: Balance the following oxidation-reduction reaction that occurs in acidic solution using the half-reaction method: - 2+ a. Cu(s) + NO (aq3  Cu (aq) + NO(g) Part of 18.32: Balance the following oxidation-reduction reaction that occurs in basic solution using the half reaction method: b. CN(aq) + MnO (aq) 4CNO(aq) + MnO (s) 2 - - The oxidation numbers for CN are C: +2, N: -3 and CNO are C: +2, N: -1, O:-2. 4. The blood alcohol (C H OH)2le5el can be determined by titrating a sample of blood plasma with 3+ an acidic potassium dichromate solution, resulting in the production of Cr (aq) and carbon dioxide. The reaction can be monitored because the dichromate ion (Cr O ) is orange in solution, and the Cr ion is green. The balanced equation is 2 7 16H (aq) + 2Cr O (2q)7+ C H OH(a2) 5 4Cr (aq) + 2CO (g) + 11H O(l) 2 2 This reaction is an oxidation-reduction reaction. What species is reduced, and what species is oxidized? How many electrons are transferred in the balanced equation above? 5. Chapter 5, Problem 44 + a little a) A balloon is filled with a gas to a volume of 7.00 x 10 mL at a temperature of 2 20.0˚C. The balloon is then cooled at constant pressure to a temperature of 1.00 x 10 K. What is the final volume of the balloon? b) What if the balloon were filled with a liquid? Would the balloon get smaller as you cooled it? Explain. Do Boyle’s law, Charles’ Law, and/or PV=nRT apply to liquids? Problem Set 5B 1. Chapter 5, Problem 68 Concentrated hydrogen peroxide solutions are explosively decomposed by traces of transition metal ions (such as Mn or Fe): 2H 2 (2q)  2H O(l)2+ O (g) 2 What volume of pure O (g),2collected at 27˚C and 746 torr, would be generated by decomposition of 125 g of a 50.0% by mass hydrogen peroxide solution? Ignore any water vapor that may be present. 2. Chapter 5, Problem 74 Urea (H N2ONH ) is 2sed extensively as a nitrogen source in fertilizers. It is produced commercially from the reaction of ammonia and carbon dioxide: 2NH (3) + CO (g)2 H NCONH2(s) + H O2g) 2 Ammonia gas at 223˚C and 90. atm flows into a reactor at a rate of 500. L/min. Carbon dioxide at 223˚C and 45 atm flows into the reactor at a rate of 600. L/min. What mass of urea is produced per minute by this reaction assuming a 100% yield? 3. a little + Chapter 5, Problem 78 a) Start with the ideal gas law, and derive an expression which relates the P and T of a gas to its density, ρ. b) Chapter 5, Problem 78 A compound has the empirical formula CHCl. A 256 mL flask, at 373 K and 750. torr, contains 0.800 g of the gaseous compound. Give the molecular formula. 4. Chapter 5, Problem 86 Consider the flask apparatus in Exercise 85, which now contains 2.00 L H at a pr2ssure of 360. torr and 1.00 L N a2 an unknown pressure. If the total pressure in the flasks is 320. torr after the stopcock is opened, determine the initial pressure of N in2the 1.00-L flask. 5. Chapter 5, Problem 94 Xenon and fluorine will react to form binary compounds when a mixture of these two gases is heated to 400˚C in a nickel reaction vessel. A 100.0 mL nickel container is filled with xenon and fluorine, giving partial pressures of 1.24 atm and 10.10 atm, respectively, at a temperature of 25˚C. The reaction vessel is heated to 400˚C to cause a reaction to occur and then cooled to a temperature at which F is a2gas and the xenon fluoride compound produced is a nonvolatile solid. The remaining F gas is 2ransferred to another 100.0 mL nickel container, where the pressure of F at 25˚C is 7.62 atm. Assuming all of 2 the xenon has reacted, what is the formula of the product?

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