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Midterm 1 Study Guide

by: Carly Rasmussen

Midterm 1 Study Guide Chem 1066

Marketplace > University of Minnesota > Chemistry > Chem 1066 > Midterm 1 Study Guide
Carly Rasmussen
U of M
GPA 3.93
Chemical Principles II
Dr. Driessen

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About this Document

Here's a quick overview of the basic kinds of problems we need to know how to solve for the midterm as well as some important relationships. Good luck!!
Chemical Principles II
Dr. Driessen
Study Guide
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This 4 page Study Guide was uploaded by Carly Rasmussen on Saturday February 14, 2015. The Study Guide belongs to Chem 1066 at University of Minnesota taught by Dr. Driessen in Spring2015. Since its upload, it has received 170 views. For similar materials see Chemical Principles II in Chemistry at University of Minnesota.

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Date Created: 02/14/15
Study Guide Key Relationships 1 Rate oc collision frequency oc collision energy oc concentration 2 Boiling point oc van t Hoff number dissociated ions 3 Pressure of gas above a solution oc solubility 4 Solubility gas inversely 0c temperature 5 krate constant controls formation of productsequlilibrium Types of problems 1 Calculating solubility a Use SKHPgas i S solubility ii KH Henry s Law Constant specific to gas and given on cover sheet iii Pgas partial pressure of gas b Example At 2500m the partial pressure of nitrogen is 0 l latm What is the pressure of nitrogen in water at 2500m and 20C i Breakdown info 1 Looking for solubility units of M 2 Given PgaS0llatm 3 On cover sheet KH of nitrogen at 20C 70 X 10394molLatm ii SKHPgaS 1 S70 X 10394molLatm0llatm cancel atm 2 S77 X 10394molL M 2 Finding Van t Hoff numberfreezing point depressionboiling point elevation a Use either AtZSKfVAtZSKb At i change in temperature ii i 39 Van t Hoff factor iii m molality of solution iv Kf freezing point constant of solvent usually water given on cover sheet v Kb boiling point constant of solvent usually water given on cover sheet b Example If the boiling of an aqueous solution of 076m KCl is 10056C What is its Van t Hoff factor What is its freezing point i Breakdown of info 1 Looking for i first 2 A t I 100 10056 I 056 3 m 076m KCl 4 Kb 0512Cm AIZJKb 1 O56Ci076m039512c m 2 i144 iii NZSKJ 1 At144076186 2 At204C 3 0C204C204C 3 Finding concentration at a given time using the halflife first order reaction a Example For the first order reaction AB the halflife is 207 minutes If the beginning concentration of A is 0250M What With its concentration be after 1 hour i First find the rate constant for the equation 0693 1 Use k Where t12 halflife and k rate constant 0693 k 0693 2 207min k 207 min k0033 ii Second find the concentration after 1 hour ALO 1 Use integrated rate law A HZ kt 5 ln Z 60 min A otz 00331hour x o025 M 2 our ln 8 A 3 198 339 ln 8 ALte139980138M 4 6 4 Conversions a Example Convert 0907M PbN032 to molality dsolu on1252gml Molar Mass of PbN0323312gmol i What is the end goal molality mol of solutekg of solvent ii Find mass of solution PbN032 1252 g solution X 1000 mL solution 1252 g solution 1 mL of solution 1 L of solution 1 L of solution iii Find mass of solute 0907 moleNo32 3312 ngNo 32 3004ngNo32 x 1 Lof solution 1mol Pb NO 3 2 l L of solution iv Find mass of solvent H20 1252 g solution 3004 g solute 9516 g solvent X 0952 kg solvent 8 V Divide moles by mass of solvent m0907moleNO32 20953mpbN032 0952 kg solvent a Example Convert 0273KClm to molarity Dsolu on1011 gL MM KCl 746gmol i What is the end goal molarity mol of solute1L of solution ii Find grams of solute m 204g KCl 2 K 0 73mol Clx lmolKCl iii Find grams of solvent 1000 g H 2 0 1k H20 8 X 1kgH20 iv Find total mass of solution solute solvent 1000g H 2 0 204g KCl10204g solution v Convert grams of solution to liters using the density of solution 1L 10204 l t39 1009L gso u ionx 10118 vi Divide moles of solute by the obtained liters 0273 mol KCl 202702 1009 L solution


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