University of Michigan, CHEM 230
Excerpt: ... r a day or so has passed work some additional problems to reinforce your understanding of the section you have been studying. From the lecture 3 6NaN3(s) + Fe2O3(s) 3Na2O(s) + 2 Fe(s) + 9N2(g) This is the reaction that inflates "air bags" in cars. Is it balanced? We need to produce 100.8 L of N2 at 273K and 1 atm. 1) How many grams of NaN3 should I use? 2) Since NaN3 is a energetic material we need to completely react the entire amount used. How much Fe2O3 do I need to sure to insure that sodium azide is the limiting reagent? Take four minutes to work through these two problems using the 5 step method. Compare your method and results with your neighbors. Ideal Gases Act Independently Since there are no interaction between the gas particles each gas particle behaves independently Partial pressures are additive Ptot = Pa+Pb+Pc Ideal gas equation for component"a" PaV = naRT Mole fractions for component"a" na/ntot = Pa/Ptot For ideal gases Components in a gas mix ...
Michigan State University, LBS 172
Excerpt: ... Concept Mapping Assignment-Due 2/2/05 Objective: Create a map that shows the information required to convert between the following concentration units: molarity, molality, mole fraction, weight percent, and parts per million (ppm). Examples: total pr ...
University of Texas, CH 53750
Excerpt: ... 1 atm at these conditions. However, if we were to isolate the hydrogen we'd find a pressure of 2.9 atm; isolating the helium and measuring the pressure would yield 7.2 atm. Note how the mixture (hydrogen + helium) has a total pressure which is equal to the sum of the individual pressures exerted by just the hydrogen and just the helium. Mathematically, we can write: PTotal = P1 + P2 + P3 + P4 + P5 + Where the subscripts represent each individual component in the mix. Using Partial Pressures An important result of Dalton's law is that if we have a gas mixture, and we know the number of moles of each gas comprising the mix, we can easily write the total pressure for the gas mixture: RT RT P T o ta l = ( n 1 + n 2 + n 3 + . . . ) = n T o ta l V V Partial Pressures with Mole Fractions We can introduce a new quantity (think of this as a concentration) called the mole fraction. Mole fractions should only be written for mixtures, as they express the moles of each indi ...
Vanderbilt, CHEM 102a
Excerpt: ... General Chemistry Lecture 102a In class notes for October 8, 2007 Chapter 5 OWL due Thursday at 11:59 pm Exam #2 a week from Thursday Dont say a word! Last Lecture Partial pressures, mole fraction Kinetic Theory (Assumptions) Today Kinetic Th ...
University of Alabama in Huntsville, CHE 441
Excerpt: ... nter the temperature and pressure. Enter the total molar flow rate. You will have to calculate this value a priori (via ideal gas law). For 'Comp Unit' select 'mole fraction'. Then enter the appropriate mole fractions for the inlet stream. Click 'OK'. 1 Now we are ready to run the simulation. Select 'run all' in 'Run' menu. If one entered all of the correct information, one should see a "Run Finished" message at lower left corner of screen. If errors exist, a window will appear which defines/describes the errors. When the simulation runs without errors, open the outlet stream. View the stream's mole fractions . Do they agree with the mole fractions indicated on the mathcad sheet for this example (website)? Now to generate a plot of mole fractions versus reactor position. Go to 'Run' menu and select 'Sensitivity Study'. Select 'New Analysis'. Enter a name for the analysis. Click on 'Edit Independent Variable'. Select 'Equipment'. Enter number given to reactor on flowsheet (in ...
Vanderbilt, CHEM 102a
Excerpt: ... General Chemistry Lecture In class notes for October 17, 2007 Exam #2 7-9pm Thursday Furman 114 Chapter 4 Acide base to Chapter 6-6 concentration units Some stuff available Units of pressure (1atm=760torr=) Units of R (0.0821 (L x atm)/(mol K) ...
E. Kentucky, CPE 211
Excerpt: ... , you were taught that: 1 mole = 6.0223 1023 molecules (Avogadro's number of a substance. And: the mass of 1 mole = Molecular Weight in g. In Chemical Engineering, we extend that definition to include other units of mass: g-mole (mol) lb-mole kg-mole (kmol) etc. How many molecules in a lb-mole? MW (g) MW(lbm) MW(kg) Table B.1 gives molecular weights for a number of compounds. If, you can't find the compound you need in Table B.1, compute its molecular weight from the compounds listed in the back cover of your book. CPE 211, F01 Lecture 4, Page 7 Example: Calculate the g-moles and lb-moles in 1.00 kg of ethane (C2H6). CPE 211, F01 Lecture 4, Page 8 Mass and Mole Fractions for n components: Mass Fraction = yi = wi n wi i =1 Where wi is the mass of component i. Mass Percent = 100% (Mass Fraction). Mole Fraction = yi = mi Where mi is the mass of component i. mi i =1 n Mole Percent = 100% (Mole Fraction). Example: CPE 211, F01 Lecture 4, Page 9 Now, we could calculate mass percent from the mass ...
Virginia Tech, CHEM 1045
Excerpt: ... Date performed: Date submitted: Instructor: Name: Partner: Title Objective A brief statement of the objective. Main point for the goal of the lab; Experimental Data List your datas in a table which should have five columns ( in right order from le ...