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Chemistry 301 Notes

by: Nhi Notetaker

Chemistry 301 Notes Chem 301

Nhi Notetaker

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Principles of Chemistry I
Dr. Jones
Class Notes
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This 3 page Class Notes was uploaded by Nhi Notetaker on Thursday September 15, 2016. The Class Notes belongs to Chem 301 at University of Texas at Austin taught by Dr. Jones in Fall 2015. Since its upload, it has received 4 views. For similar materials see Principles of Chemistry I in Chemistry at University of Texas at Austin.

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Date Created: 09/15/16
What is gas?    A gas can be made of atoms or molecules or mixtures.     Gases have low density, low viscosity, expand and contract with changes in temperature and  pressure, distributes uniformly throughout a container.     Pressure = force/area    1 atm = 760 mmhg = 760 torr    Pascal (Pa) 1 N/m^2 (recommended IUPAC unit)    1 atm = 101325 Pa    1 bar = 100,000 Pa    Pounds per square inch (psi), air pressure at sea level is (14.7psi)    Boyle’s Law  Pressure is inversely proportional to volume at constant temperature.  P*V=k(constant)  P1*V1=P2*V2    Charles Law  Volume directly proportional to temperature at constant pressure.   V/T= k (constant)  V1/T1=V2/T2    Avogadro's Law  Volume of gas is directly proportional to the amount of gas (in moles) at constant  temperature and pressure. Equal volumes of all(ANY TYPE) gases, at the same temperature  and pressure, have the same number of molecules.     Combined gas law  PV/T=k (constant)  As long as the number of moles is constant k will be a true constant value.   P1V1/T1=P2V2/T2    Ideal Gas Law  PV=nRT  R=0.088206 L atm/(molK)  R= 8.314 J/(molK)  R=0.08314 L bar/(molK)  R=1.987 cal/(molK)  R=8.314 J/(molK)  R=8.314 m^3*Pa/(molK)  R=62.36 L*torr/(molK)    Mass density: MP=pRT    Standard Conditions aka State functions  STP­ 0 degree celcius (273.15K), 1 atm  SATP (standard ambient temperature and pressure)  IUPAC (international union of pure and applied chemistry)  25 degree celsius (298.15K), 1 bar pressure     Standard molar volume  Volume of an ideal gas at STP­ Approx. 22.4 L  At other temps and pressure use PV=nRT    Number density (avogadro's law)  Number of particles present in a given volume (mol/L)  At constant temp. ­number density governs pressure  Different gasses with same P,V, T have same number density  n/V=P/RT  Not related to the identity of actual gas    Mass density (p)  Number moles=mass/molar mass and density(p) =mass/volume  M(molar mass)=d(p)RT/P  Used to find molecular weight of a gas from density, pressure and temperature  Or find the density of a gas from its molecular weight, temperature, and pressure  Molecular weight is directly proportional to mass density      Number density: # moles/volume  Molar volume: volume/# moles    # of moles = mass/molecular weight  Density = mass/volume  PV=nRT  (molecular weight)n/V=P/RT(molecular weight)    Ex. balloon of helium and argon, same number particles(V,P,T) and number density, different  mass density because argon is heavier (mm)    Partial Pressure  An idea, not an actual measurement  Total pressure = a sum of pressure  P(total)= P(a)+ P(b) + P(c)....   P(total) = n(moles) RT/ V  P(a) = n(a)RT/V    Partial pressure of gas (a) = (mole fraction of A)(total pressure)  Mole fraction (Xa) = # of moles A/ total # of moles 


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