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Chemistry Wee3 Notes

by: Mena Ibrahim

Chemistry Wee3 Notes Chem001A

Mena Ibrahim
GPA 3.6
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About this Document

Covers Stoichometry, finding limiting reagents along with a few examples.
General Chemistry
Dr. Harman
Class Notes
Chem, Chemistry, Stoicheometry




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This 6 page Class Notes was uploaded by Mena Ibrahim on Friday October 14, 2016. The Class Notes belongs to Chem001A at University of California Riverside taught by Dr. Harman in Fall 2016. Since its upload, it has received 3 views. For similar materials see General Chemistry in Chemistry at University of California Riverside.


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Date Created: 10/14/16
Mena Ibrahim  Stoichiometry Conversion qualitative terms ­ i. Balance chemical reactions  i. (to give mole ratios, try to balance the carbons first)  ii. Balance elements that come up once,  i. and those that come up at  each side of the reactions.  iii. Must know how to convert mass to moles and vise versa.  iv. When you have the reaction in moles, you can find the moles of the  missing chemical that you need and be able to reconvert the mole to  mass to find how much you need to make the chemical reaction  balanced.  MUST FIND THE LIMITING REAGENT    What is it?  ­ It determines the amount of product that will be produced. (it is 100% consumed and once it runs out, the reaction stops.)  i. If you have only one reactant, that isn’t called the limiting reactant. ii. You Need more than one reactant in order to determine which single  reactant is  heavily used.               HOW TO FIND LIMITING REAGENT Step 1: Balance the equation.  (2)H2 + O2 ­> (2) H2O Step 2: Use calculator on midterm to determine the limiting reagent.                 Check if you have more reactants than product which will be explained in step  4.  Step 3:     Q) How much product is obtained from the reaction of 20.00g SO3 and             10.00 H2O             (evaluate assuming that you have infinite amount of the other reactants) Step4: Convert all masses to moles and calculate the limiting reagent for both  reactant.  amount reagent (reactant) *   molar mass  *   mole ratio      *     mass of product            20.00 SO3 * (mole/80.06g)  *  (1/1) (H2SO4/SO3) * (98.07/mole  H2SO4)   = 24.5grams  2  Reactant   10.0g H2O (mole/18.0g) * (H2SO4/H20) * (98.07g/mole) = 54.7g  Step 5: Now look for which reagent leads to the LEAST AMOUNT OF  PRODUCT!!!!!    So the answer for this example would be SO3 will be your limiting reagent,  because it would be the first reagent that would be used up before H2O.    PERCENT YEILD THEORETICAL YIELD is what you calculate without any errors.     (Most ideal amount of yield if there is no error)  ACTUAL YIELD ­is when you actual perform the reaction in a real life lab.  (this includes human errors, systematic error.  a) this should never be over 100% because your theoretical yield is when  there has been no type of error occurring at all. But in reality there will be some minor errors.  Example    Al reacts with Br Liquid, producing AlBr3. In one experiment, 6.0g  Al reacts with an excess of bromine to yield 50.3g aluminum bromide. Calculate the theoretical and percent yields.  Step 1: Come up with a chemical reaction      (2) Al + (3) Br2 —> (2) AlBr3  Step 2:Calculate the Theoretical Yield      6.0g Al * (mole/ 26.98g) * (2AlBr3)/2Al) * 266.69g/ mole = 59g Now since you have been given the actual percent Step 3: Calculate the percent yield         Actual / Theoretical       50.3g/ 59g *100= 85% APPLICATION PROBLEM 1)   You are given a liquid smile that contains methanol (C3OH), ethanol  (C2H5OH) or a mixture of both. You see combustion analysis of a 0.336g  sample and obtain 0.462g of CO2. What did you learn about your sample?  Solution:  1. balance the  equation (2) H3COH * (3) O2 —> (2) CO2 + 4H2O  2. Calculate the limiting reagent:  0.336g H3COH * (mol/32.04g)  (1/2 mole ratio) * product mass = .462g Senario 2:    balanced equation: should have  1mole ethanol + 3mole O2 —> 2 mole CO2 + 3 mole of H2O 0.336g * mole/46.07 of ethanol * 2/1 mole ration * 44g of product = 0.641g.  the amount is 0.641g ­ which is not the answer so we know even if you  combine them they will still be off so the correct answer is the first scenario.  Answer: Only Methanol


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