Principles of Chemistry 2 Hybrid
Minneapolis Community and Technical College

Spring 2018

           ...Course Lectures
              ...Lab Manual
                ...NEW: Grades (2/7/18)
                  ... Lab Grades

                           Campus Map

Withdrawing?...Click HERE first.

Schedule a tutor.
Office Hours (S-3580)
Tuesday:    12:00 - 2:00 PM
Wednesday: 2:00 - 4:30 PM
Kirk's Weekly Schedule
 Online Office Hours:    TBA   
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Instructor: Kirk Boraas


E1 Online D2L    2/5  or  2/6     7 - 9 PM
E2 On-Campus    3/13                6 - 9 PM   Rm S-2400
E3 Online D2L     4/9  or  4/10   7 - 9 PM
E4  On-Campus   5/3                  6 - 9 PM  Rm L-3000
Optional Final      5/9                  6 - 9 PM  Rm S-3400

Exams and Answers

Previous Daily Postings and Videos

  Weeks 1 & 2         
Weeks  3 & 4        NEW:  Weeks 5 & 6     Weeks 7 & 8      |  Weeks 9 & 10     Weeks 11 & 12     Weeks 13 & 14     Weeks 15 & 16

This is not an online course.
  Campus visits are required (weekly labs and periodic exams)

February 19, 2018   Monday   Week 7

Le Chatelier's Principle

     .....know the ways an equilibrium can be shifted left and right
          (Changes in volume, pressure, temperature and concentration)

     ....predict how increases or decreases in reactant or product concentrations
         affect the position of the equilibrium

     .....predict how increases or decreases in reactant or product pressures
         affect the position of the equilibrium

     .....predict how increases or decreases in temperature affect the position
          of the equilibrium

     .....use observed equilibrium shifts to identify reaction as exothermic
          or endothermic.

Study questions.

Which of the below are ways that allow you to recognize equilibrium?    (Source)
     a. Constant Temperature    b. Constant Color     c. Constant Pressure

2. Consider the following equilibrium reaction:    Fe3+(aq)      +     SCN-(aq)   
↔     FeSCN+2(aq)                   (Source)
                                                                               Colorless            Colorless          Deep Red

i.   Adding more Fe(NO3)3  will shift the reaction _______________ and produce more _____________________
     ii.   Adding AgNO3 to the test tube removes SCN- from the reaction causing the reaction to shift ________________ and produce more ___________.
     iii.  If the reaction container is placed in an ice bath the mixture turns darker red.  We conclude that the reaction is ...
            a.   Exothermic      b. Endothermic

3.  How will an increase in pressure affect the following equilibrium reaction:   N2O4(g)    
↔     2 NO2(aq)             (Source)

     a. Reaction shifts right to form more products
     b. Reaction shifts left to form more reactants.
     c.  This equilibrium is unaffected by changes in pressure.

4. In the reaction, CO (g) +    NO
2 (g)     ↔   CO2 (g) +    NO (g), which of the following changes would result in the formation of more
    products at equilibrium?

     a. increasing the pressure
     b. removing CO(g) from the reaction
     c. adding NO2(g) to the reaction
     d. adding CO2(g) to the reaction
     e. None of the above.

Answers:  Click and drag in the space below.

1. a, b, and c     
2. i.  right, products   ii. SCN- levels drop, reaction shifts left   iii.  a. Exothermic
3. b
4. c