Chem 1320 1st Edition Lecture 10Outline of Last Lecture I. Word ProblemOutline of Current Lecture I. DilutionII. GasesIII. AssumptionsIV. Important VariablesCurrent LectureI. Dilution Dilution is when you add solvent to a solution. Example: Prepare 60mL of 0.2M HNO3 from stock of 4M HNO3(4M) (XL) = (0.2M)(0.06L) X= 3.0 x 10-3L or 3mL3mL of 4M HNO3 needed with 57mL of water - This will give you 60mL of the solutionEquation: M1V1=M2V2II. GasesGasses are comprehensible and occupy the volume of their containers. The pressure goes up and the volume goes down. This is called Boyle’s law, V= 1/P. Volume of a gas can be changed with temperature. This occurs when the temperature and the volume both go down. This is known as Charles’ law. Gas also has a low viscosity; easy flow. Gases have a low density and mix readily. Ideal gases are applied independently of chemical identity of the gas. These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.III. Assumptions Some assumptions are that gases are composed of non- interacting parties. Also, that all particles are continuously moving (fast). Volume of the gas particles are small compared to a container which is also an assumption. IV. Important VariablesP= pressure (atm)V= volume (L)T= temp (K) + 0˚C = 273.15K, 100 ˚C = 373.15Kn= moles (mol) The ideal gas equation (law): PV= nRT R= gas constant = 0.08206 (L)(atm)/ (mol)(K)Changing conditions: - Condition One: P1V1=n1RT1 P1V1 = n1T1- Condition Two: P2V2=n2RT2 P2V2
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