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Week 11, Ch. 11/12

by: Bianca Notetaker

Week 11, Ch. 11/12 CHEM 111 001

Bianca Notetaker
GPA 3.0
Elements Of General Chemistry

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About this Document

Introduces chapter 12 and wraps up chapter 11 contents
Elements Of General Chemistry
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This 3 page Study Guide was uploaded by Bianca Notetaker on Tuesday November 3, 2015. The Study Guide belongs to CHEM 111 001 at University of New Mexico taught by smith in Summer 2015. Since its upload, it has received 42 views. For similar materials see Elements Of General Chemistry in Chemistry at University of New Mexico.


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Date Created: 11/03/15
1132015 OneNote Online Wednesday October 28 2015 1001 AM Concentrated and diluted solutions 0 Concentrated solution has more particles of solute per unit of mass 0 Dilute solution has fewer particles of solute per unit of mass 0 M molV Mol mol of solute dissolved V total volume of solution in liters 0 Solving for different variables MmolV MolMxV VmolM Molaritypractical calculations 0 Making a solution at a particular molarity Mol M x V o Dilution calculations go from a stock concentrated solution to a working diluted solution M1V1 M2V2 Solution mole ratios and ion molarity o The dissociated ions may be in a different ration than the parent compound 0 The product of neutralization problem is always a water a salt Other concentration units 0 Percent by mass Mass of solute total mass solution x 100 0 Percent by volume volume of solute total volume solution x 100 0 Just like with empirical formulas wherever you have percentages assuming you have 100 total is a good way to get initial amounts 0 Parts by mass mm or ww 0 Parts by volume vv 0 Mixed case mv Collocation properties 0 Many physical properties change based solely on the number of solute particles in the solution including Vapor pressure lowering Freezing point depression Boiling point elevation Osmotic pressure 0 You must distinguish between solutes that do and do not dissociate httpsonenoteofficeappsivecomoonenoteframeastFiSDE50F6024D8D962E0417ampHemuampC5810SN2SKYWACWSHIampuienUSamprs 11 1132015 OneNote Online Gases Monday October 26 2015 1003 AM Pressure in terms of atoms and molecules 0 Gas pressure varies with temperature container size and the amount of gas particles Higher temperature faster the molecules move The smaller the area the greater the pressure 0 Pressure force area PFA 0 SI Units Force 1 Newton N kg x ms2 Area m2 Pressure Nm2 1 pascal 1 Pa o 1 atmosphere 760 torr 760mmHg101325 Pascal Atmospheric pressure 0 Higher up you are the less atmospheric pressure there is Pressuremeasurement 0 Mercury is he dentist liquid at room temperature 13534gcmA2 0 Early empirical studies V and T Law relationship Direct relationship Charles Law V X T V T Direct Const P n Avogadros V X n V n Direct Const T P Law n moles Boyles Law V and V Inverse Const T n P 1P Ideal gas law 0 V nTP All the laws above combined 0 VRnTP R constant of proportionality quotideal gas constantquot 0 PV nRT Ideal gas law IGL o R PVnT 008206 L x atm mol x K Using the ideal gas law a Pressure should always be in atmospheres b Temperature should always be in kelvin c Volume must be in Liters cl Amount must be in moles Implications of the ideal gas law 0 STP standard temperature and pressure vol of 1 mole of Ideal gas 0 Any ideal gas at STP T 27315 K 0 Celcius Both gt 224 Lmol at STP V 224 L httpsonenoteofficeappsIivecomoonenoteframeastFiSDE50F6024D8D962E0417ampHemuIampC5810SN2SKYWACWSHIampuienUSamprs 12 1132015 OneNote Online P 1 atm Whenever you have an ideal gas at STP this relationship applies 1 mol of any ideal gas will 224 L of STP InitialFinal calculations 0 PVnT R always constant Molar mass and the IGL 0 Mass x 1molar mass moles Or mMM n o If you substitute this into the IGL you get a new expression PV mMMRT gt MM mRTPV 0 Substitute it into the density equation D m nRTP o STP conditions x224 httpsonenoteofficeappsivecomoonenoteframeastFiSDE50F6024D8D962EO417ampHemuampC5810SN2SKYWACWSHIampuienUSamprs 22


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