1. CaCO3 (s)   CaO (s) + CO2 (g)
7:16 #14
ANALYZE : question asks for a equilibrium shift resulting from a pressure change.
THEORY: LeChatelier : Increasing pressure goes to side of least moles OF GAS.
APPLY: the answer is choice 2, there are no gasses on the left, increasing pressure goes there.
CaCO3 (s)   CaO (s) + CO2 (g)
7:16 #15
ANALYZE: Temp is increased changed on a system at equilibrium.
THEORY: Increasing temp reverses an exothermic reaction, forwards an endothermic one.
APPLY. This reaction is endothermic (heat is written on the left)
2HBr kJ   H2 + Br2
HEAT
-2X X X choice 1
Increase T, heat enters on left, EQ shifts to the right,

2. Increase N2, enters on left, EQ shifts to the right,
7:16 #16
ANALYZE : question asks for a equilibrium shift resulting from a increase of N2 change.
THEORY: LeChatelier : Increasing on one side shifts to the opposite side.
APPLY: N2 is on the left. Increasing it shifts to the right.
N2 (g) + O2 (g)  2 NO (g)
WHAT THE SYSTEM WILL DO AFTER STRESS IS ADDED.
-X X X
Increase N2, enters on left, EQ shifts to the right,
7:22 #34
ANALYZE : about an equilibrium pressure increase stress.
THEORY: LeChatelier : Increasing pressure drives to the side of least moles OF GAS.
APPLY: moles on each side are equal, no effect! Ans C no change
N2 (g) + O2 (g)  2 NO (g)
1 mole = moles

3. 2 H2 (g) + O2 (g) 2 H2O (g) + HEAT
7:22 #35
ANALYZE : Heating a systemat equilibrium.
THEORY: Heating and exothermic reaction reverses it.
APPLY: This reaction will be reversed as you are heating exo reaction, heat enters on the right and shifts left.
2 H2 (g) + O2 (g) 2 H2O (g) + HEAT
+2X X X : choice#4
HEAT
INCREASING T, heat enters on RIGHT, drives (LEFT).
7:22 #39
ANALYZE :Common Ion Effect, adding Cl-.
THEORY: LeChatelier : on right shifts left .
APPLY: In this reaction, Cl- enters on right, reaction shifts LEFT.
AgCl(s) (g)   Ag+ (aq) + Cl- (aq)
+2X X X : choice #2
INCREASING Cl- , enters RIGHT and shifts LEFT.

4. 7:19 #9
ANALYZE: A + B  C + energy IS EXOTHERMIC, heat on right, BEING GIVEN OFF (EVOLVED).
THEORY: In an EXOTHERMIC REACTION the products have LESS POTENTIAL ENERY content then the REACTNTS, the rest is lost from the reaction as heat.
APPLY: In the reaction kinetics energy graph, the products will be at a LOWER level than reactants. CHOICE 2
A + B C
REACTANTS
PRODUCTS

5. 7:19 #10
ANALYZE :Potential energy diagram
THEORY: The products are at lower energy level in an exothermic reaction.
APPLY: In the diagram below, the products are at a lower energy level than the reactants, the difference is evolved as heat (kinetic energy). The reaction loses potential energy as the kinetic energy of heat.
A + B AB
REACTANTS
PRODUCTS

6. A 7:20 #16 and 17 ANALYZE : Given a potential energy graph
THEORY: If the products are at a higher energy level than the reactants, the reaction is ENDOTHERMIC, heat is stored in the products as potential energy.
APPLY: The products are at a higher level in this graph, ENDOTHERMIC and energy is gained (absorbed) by the system.
ACTIVATED COMPLEX
FORWARD ACTIVATION ENERGY A
PRODUCTS
ANSWER: 16 IS ARROW A, FORWARD ACTIVATION.
17 IS ENDOTHERMIC AND HEAT IS ABSORBED CHOICE 4
REACTANTS