Honors Chemistry (Period 2,4) (Chatsworth Charter High School & G+STEAM Magnet Center) //www.chatsworthhs.org/apps/classes/736809/assignments/ Class Name: Honors Chemistry (Period 2,4) Instructor(s): Steve West en-us SchoolSitePro <![CDATA[Due: 06/06/2016]]> //www.chatsworthhs.org/homeworkItem4344309 //www.chatsworthhs.org/apps/classes/736809/assignments/ Here are two ICE box equilibrium questions for you:
 
  1. Suppose that 2.00 moles of HCl in a 1.00L glass flask slowly decomposes into H2 and Cl2. When equilibrium is reached, the concentration of H2 is 0.214 M. Determine the equilibrium concentrations and Keq?

     

                                                    2 HCl (g)   ↔  H2 (g)   +   Cl2 (g)

     

  2. 3.00 moles of NO(g) are introduced into a 1.00-Liter evacuated flask. When the system comes to equilibrium, 1.00 mole of N2O(g) has formed. Determine the equilibrium concentrations of each substance. Calculate the Keq for the reaction based on these data.

     

     2N2O(g) + O2(g) ↔ 4NO(g)


]]> Thu, 02 Jun 2016 14:54:58 PDT <![CDATA[Due: 06/02/2016]]> //www.chatsworthhs.org/homeworkItem4342752 //www.chatsworthhs.org/apps/classes/736809/assignments/ The attached review guide is designed for general chem.  It is good practice, but doesn't cover the higher level concepts
]]> Tue, 31 May 2016 10:23:39 PDT <![CDATA[Due: 05/31/2016]]> //www.chatsworthhs.org/homeworkItem4341456 //www.chatsworthhs.org/apps/classes/736809/assignments/ Complete the attachment: Kinetics Review Part I
]]> Thu, 26 May 2016 14:29:29 PDT <![CDATA[Due: 05/26/2016]]> //www.chatsworthhs.org/homeworkItem4339718 //www.chatsworthhs.org/apps/classes/736809/assignments/ Complete (as much as possible) the attached file practicing reaction mechanisms.  Also attached here is the "Method of Initial Rates" worksheet we worked on in class last Friday.
]]> Tue, 24 May 2016 14:51:07 PDT <![CDATA[Due: 05/18/2016]]> //www.chatsworthhs.org/homeworkItem4331807 //www.chatsworthhs.org/apps/classes/736809/assignments/ Assessment today. Topics include:
  • equations
  • net ionic equations
  • models
  • applied stoichiometry problem
You should study your homework from May 12, May 6, May 2, and April 28. 
 
Here is the problem worked on in class on Monday, May 16:

Aluminum metal can be oxidized by hydrochloric acid solution. Determine the minimum volume of 0.75 M HCl required to completely oxidize 1.00 gram of aluminum metal.


]]> Mon, 16 May 2016 14:35:07 PDT <![CDATA[Due: 05/17/2016]]> //www.chatsworthhs.org/homeworkItem4331809 //www.chatsworthhs.org/apps/classes/736809/assignments/ Tutoring after school today
]]> Mon, 16 May 2016 14:35:29 PDT <![CDATA[Due: 05/12/2016]]> //www.chatsworthhs.org/homeworkItem4325769 //www.chatsworthhs.org/apps/classes/736809/assignments/ This assignment is actually due on the day of the assessment, which has been moved to Wednesday May 19th. 
 
solve the following applied stoichiometry problems:
  1. Calcium is an important component of bone tissue. Assume that artificial bone is composed of calcium chloride.  5.00 grams of an artificial bone sample is dissolved in acid and the solution is reacted with excess sodium sulfate to precipitate all of the calcium.  1.56 grams of solid precipitate is recovered.  Determine the mass percent of calcium chloride  in the bone sample. (Write models for this one too).
  2. An unknown rock sample contains aluminum carbonate.  2.50 grams of the sample is reacted with excess nitric acid (HNO3, strong acid).  1.10 grams of carbon dioxide gas is released.  Determine the mass percent of aluminum carbonate in the rock sample.
  3. Phosphoric acid (H3PO4) is a weak acid that helps give Slurpees their tangy taste.  125.0 ml of a certain Slurpee is titrated with 0.0100 M NaOH to its equivalence point (neutralize all of the acid). 5.50 ml of NaOH is required for the titration.  Use this data to calculate the concentration of H3PO4 in the Slurpee.
Please make sure to write net ionic equations in addition to balanced equations for each question above.

]]> Thu, 12 May 2016 10:52:11 PDT <![CDATA[Due: 05/06/2016]]> //www.chatsworthhs.org/homeworkItem4319641 //www.chatsworthhs.org/apps/classes/736809/assignments/ solve the applied stoichiometry problems:
  1. Zinc (II) phosphate is an important substance used in coating metal surfaces (especially cars) to prevent corrosion.  Solid zinc (II) phosphate can be precipitated out of solution by reacting zinc nitrate and potassium phosphate solutions.
    • write a balanced equation and net ionic equation for the precipitation reaction.  Show models for the net ionic as well.
    • calculate the mass of solid zinc (II) phosphate that can be expected when 150.0 ml of 2.00 M zinc nitrate reacts with 150.0 mL of 1.25 M potassium phosphate. (This is a problem where we need to figure out the limiting reactant.  We did a similar problem on April 22nd.  You may want to check your notes for help).
  2. Sodium fluoride is a common active ingredient in toothpaste.  Fluoride ions can be formed through a single replacement reduction of fluorine gas (F2) by chloride ions which get oxidized to chlorine gas (Cl2) in solution.  {Note that this is not a likely mode of making fluoride for toothpaste.  Its not real safe}.  Consider the reaction: sodium chloride reacts with fluorine gas to form sodium fluoride and chlorine gas.
    • write a balanced equation and net ionic equation for the reaction.  show models for the net ionic equation as well.
    • calculate the concentration of fluoride ions formed in a solution where excess fluoride gas is pumped into 100.0 ml of a 1.50M sodium chloride solution.

]]> Thu, 05 May 2016 15:21:34 PDT <![CDATA[Due: 05/04/2016]]> //www.chatsworthhs.org/homeworkItem4314689 //www.chatsworthhs.org/apps/classes/736809/assignments/ We are beginning a study of reaction rates (how fast or slow a chemical reaction proceeds, and the factors affecting rate).  For homework, read section 17.1a-c from your textbook and complete questions (1-11) from the Chapter 17 file attached at the right.
]]> Mon, 02 May 2016 14:06:34 PDT <![CDATA[Due: 05/02/2016]]> //www.chatsworthhs.org/homeworkItem4310749 //www.chatsworthhs.org/apps/classes/736809/assignments/ Solve the following stoichiometry problems:
  1. A waste solution of lead (II) nitrate from a manufacturing plant is accidentally discharged into a local water supply. 250.0 ml of the polluted water is reacted with excess potassium chloride to precipitate the lead (II) ions.  13.9 grams of precipitate is recovered after filtering. 
    • write the balanced equation and net ionic equation
    • write models for the net ionic equation
    • calculate the concentration of lead ions in the 250.0 ml polluted water sample
  2. 200.0 ml of 1.00 M HCl is required to completely extract all the nickel (II) carbonate from 17.9 grams of an ore sample in an acid carbonate reaction.
    • write the balanced equation and net ionic equation
    • write models for the net ionic equation
    • calculate the mass of nickel (II) carbonate and the percentage of nickel (II) carbonate in the ore sample
  3. Carbonated sodas are formed by pumping carbon dioxide into the flavored water.  Carbon dioxide will react with the water to form carbonic acid (a weak acid).  In order to determine the concentration of carbonic acid in a carbonated drink we can titrate a sample with a strong base like sodium hydroxide.  Assume that it takes 15.0 ml of 1.50 M NaOH to completely neutralize 30.0 mL of a carbonic acid (H2CO3) solution. Its an acid-base neutralization reaction.
    • Write the balanced equation and net ionic equation (remember carbonic acid is weak)
    • Calculate the concentration of the carbonic acid solution

]]> Thu, 28 Apr 2016 15:39:12 PDT