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Week 5 Chemistry Notes

by: Amelia

Week 5 Chemistry Notes CHEM 1127Q-011


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9/26 and 9/28 notes. On Monday we started Chapter 4, we learned how to balance chemical equations. On Wednesday we went over three review problems for the exam, I copied them down below. Good luck ...
General Chemistry
Dr. Cady
Class Notes
General Chemistry, Balancing Equations
25 ?




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This 3 page Class Notes was uploaded by Amelia on Wednesday September 28, 2016. The Class Notes belongs to CHEM 1127Q-011 at University of Connecticut taught by Dr. Cady in Fall 2016. Since its upload, it has received 17 views. For similar materials see General Chemistry in Chemistry at University of Connecticut.


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Date Created: 09/28/16
9/26  Chapter 4­ Stoichiometry and Chemical Reactions    Chemical Reactions  1) What are chemical reactions?  a) When two or more substances interact with each other to form something new  b) There are dozens of different classifications of chemical reactions  c) Rather than classify them by how reaction happens sometimes classify by what happens.  2) Evidence of chemical reaction  a) Precipitation­ solid formed from a clear solution (cloudy)  b) Gas evolution­ gas bubbles appear   c) Give off heat or light  d) Change in temperature or energy  e) Change of odor   3) Balancing chemical reactions  a) Everything in reactant has to end up in product.  b) Reactant(s) → Product(s)  c) Example:  i) C​3​​ 8​​  2​CO​ +H​ O2​ 2​ ii) C​3​​ 8​​  2​​3CO ​ ​2​H​ 2​ iii) C​3​​ 8​​  2​CO​ +4 2​ ​ H​2​  iv) C​3​​ 8​5O​ ​2​→3CO ​ 2​+4H​ O2​ 4) Solubility and compounds dissolved in water  a) Many Ionic compounds dissolve in water… but some don’t  b) If things dissolve they are soluble  c) If things don’t dissolve they are insoluble   d) Water stabilizes Ions, makes them split from their pair to “hang” with water molecules  5) Precipitation Diagram  a) Table 4.1 in book­ shows what normally does and does not dissolve, plus exceptions  i) Anything in group one is soluble  ­​ ­​ ­​ ii) Some halide atoms (Cl​, Br​, I​) but not all.  iii) Acetate, bicarbonate, nitrate, chlorate and most sulfates.  iv) Compounds containing carbonate, chromate, phosphate, and sulfide ions are not  usually soluble . Also hydroxide ions .  v) Check the book for this one!  6) Net ionic equation  a) Just like a chemical equation only we show all the ions separately and then eliminate ones  thats are inactive/do not react.   b) The ones that react are called spectator ions.  c) Note­ the ​  (aq)​ dissolved in water    9/28  Exam 1 Review    ­ Office Hours­ Thursday 11:30­12:30 A405   ­ BRING: A pen (black or blue), #2 pencil, and ID  ­ Grades are 50­50 multiple choice and long answer   ­ 19 multiple choice questions and 10 ‘long’ answer    1) An unknown element (X) forms a compound with the formula XBr​ . If the compound contains  3​ 81.1% Br by mass, what is the molar mass of the unknown element? What is the identity of the  element?  a) Assume 100g, so Br is 81.1g  b) 100g ­ 81.1g → 18.9g X  c) 81.1g/79.90g/mole = 1.015moles Br   d) 1.015moles Br × 1X/3Br = 0.338moles of X  e) 18.9g/0.338moles = 55.917g/mole   f) 55.917g/mole → Fe, Iron  g) FeBr​  3   2) When 2.56 grams of iron is heated in air it forms an oxide that weighs 3.66 grams. What is the  empirical formula or iron oxide?  a) Fe​ O​    x​ y b) Fe → 2.56 grams  c) 3.66g (FeO) ­ 2.56g (Fe) = 1.10g (O)  d) Fe: 2.56g/55.85g/mole = 0.04588moles Fe   e) O: 1.10g/15.999g/mole = 0.06875moles O  f) 0.06875moles/0.04588moles ≈  1.5×2 = 3  g) 0.06875moles/0.06875moles ≈  1×2 = 2  h) Fe​ O​   2​ 3   3) You have a stock solution containing 0.650M AlCl​ . You add the prope3​amount of this stock  solution to a beaker to create 500mL of a 0.250M Cl​ solution. How much water do you have to  then add to the solution to attain proper volume and concentration?  a) Start: 0.650M/L of AlCl​   3 ­ b) Goal: 500mL of 0.250M Cl​   ­​ ­ c) 0.650M/L of AlCl​ × 3Cl​/13lCl​  = 1.95M Cl​3​ d) 1.95M(L) = (500mL)(.250M)  e) L = .0641 or 64.1mL  f) 500mL ­ 64.1mL = 436mL H​ O added  2​


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