DIRECTIONS:

1.     Select a new page in your Spiral lab notebook.

2.   Press hard (with a blue or black pen only – NO PENCIL OR FELT TIPPED PEN) when writing in your Spiral lab manual.

3.   Fill in the top portion of the first page only. Take the following steps:

     step 1 – print your last name followed by printing your first name in the box entitled NAME;

     step 2- Place the name Chemistry Chapter 17 Overview in the box entitled EXPERIMENT/SUBJECT; step 3 – leave EXP NUMBER blank; step 4 – Place the due date 11 APRIL 2008 in the box entitled DATE; step 5 – leave LAB PARTNER and LOCKER/DESK NO. blank; step 6 – place Chemistry period ___, what number? ___ (press hard) in the box labeled COURSE AND SECTION NO.

4.     Read Chapter 17 and summarize what you read using this outline as a guide.

5.   Chapter 17 Overview is due: FRIDAY 25 APRIL 2008

 

á       REMINDER – GRADING SYLLABUS: BASED UPON CLARITY AND NEATNESS

1.     A = THREE PAGES

2.     B = TWO PAGES

3.     C = ONE PAGE

        *********************** CHAPTER 17   OUTLINE ***********************

á       REACTION RATES AND EQUILIBRIUM

-        THE TYPICAL COLLISION MODEL INCLUDES THE FOLLOWING ACTIVITIES:

1)               REACTIONS MUST COLLIDE TO REACT.

2)               THE TERM ÒACTIVATION ENERGY, Ea, IS A CERTAIN THESHOLD ENERGY, THAT MUST BE SUPPLIED BY THE COLLSION OF COMPOUNDS/ATOMS TO OCCUR.

-        A CATALYST IS INVOLVED IN BRINGING ABOUT COLLISIONS:

1)     IT SPEEDS UP THE REACTION  WITHOUT BEING CONSUMED

2)     IT PROVIDES A PATHWAY FOR THE RECATION THAT REQUIRES A SMALLER  Ea ( ENERGY OF ACTIVATION).

3)     ENZYMES ARE USED AS BIOLOGICAL CATALYSTS.

-        CHEMICAL EQUILIBRIUM IS ESTABLISHED WHEN A CHEMIUCAQL REACTION IS CARRIED OUT IN A CLOSED CONTAINER:

                               1) THE FORWARD RATE EQUALS THE REVERSE RATE

                               2) IN HOMOGENEOUS REACTIONS ALL REACTANTS AND PRODUCTS ARE

                                    IN THE SAME PHASE.

                               3) IN HETEROGENEOUS REACTIONS ONE OR MORE REACTANTS OR PRODUCTS

                                   ARE IN DIFFERENT PHASES.

 

á       CHARACTERISTICS OF EQUILIBRIUM

-        THE EQUILIBIRUM EXPRESSION (K) IS  BASED UPON THE LAW OF CHEMICAL EQUILIBRIUM:

1)             FOR A TYPICAL REACTION: 3Mg(NO3)2 + 2AlCL3 ---ˆ 3MgCL2  + 2Al(NO3)3

2)     THE EQUILBIRIUM WOULD BE K = PRODUCTS    =   [MgCL2 ]3 [Al(NO3)3 ]2

                                                                REACTANTS      [Mg(NO3)2 ] 3    [AlCL3 ]2

 

á       TITRATIONS AND BUFFERS

-        Le CHATELIERÕS PRINCIPLES STATES THAT WHEN A CHANGE IS IMPOSED ON A SYSTEM AT EQUILIBIRUM THE POSITION OF THE EQUILIBIRUM SHIFTS IN THE DIRECTION WHICH REDUCES THE EFFORT OF THAT CHANGE.

-        THE EQULIBRIUM  CONDITIONS ALSO APPLY TO A SATURATED SOLUTION CONTAINING EXCESS SOLIDS, MS(S) OR  AgCL(S) .

-        KSP =[ Ag 1+] [CL1- ]

-        THE VALUE OF HE KSP CAN BE CALCULATED FROM THE MEASURED SOLUBILITY OF MX (S) .