1. Chapter 18 – Reaction Rates and Equilibrium
Jeopardy
Chapter 18 – Reaction Rates and Equilibrium

2. Entropy and Free Energy Le Chatelier’s Principle
Rates of Reactions
Equilibrium
Entropy and Free Energy
Le Chatelier’s Principle
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3. The rate of a chemical reaction may be increased by increasing
Temperature or concentration of reactants
The rate of a chemical reaction
may be increased by increasing
the _______ and / or ________.
Row 1, Col 1

4. When a reaction reaches equilibrium,
They are equal.
When a reaction reaches equilibrium,
what can you say about the rate of
the forward reaction and reverse
reaction?
1,2

5. What is the name and the symbol of the term used to describe the
Entropy (S)
What is the name and the symbol of
the term used to describe the
‘disorder’ of a process?
1,3

6. Decreasing the temperature of the following reaction at equilibrium
Left Shift
Decreasing the temperature of the
following reaction at equilibrium
will cause it to shift in which
direction?
N2(g) + 3H2(g) + Energy  2NH3(g)
1,4

7. As the particle size of a reactant decreases, the rate of reaction
Increase
As the particle size of a reactant
decreases, the rate of reaction
will __________.
2,1

8. What can you conclude about a chemical reaction that has reached
Reactants are favored at equilibrium.
What can you conclude about a
chemical reaction that has reached
equilibrium were the equilibrium
constant (Keq) is less than one?
2,2

9. Is there an increase or decrease in
The entropy in the following process?
CaCO3(s)  CaO(s) + CO2(g)
2,3

10. What will happen to the position of the
It will shift to the left.
What will happen to the position of the
equilibrium when the the pressure is raised
on the following chemical reaction?
PCl5(g)  PCl3(g) + Cl2(g)
2,4

11. It lowers the activation energy. How does a catalyst speed up a
chemical reaction?
3,1

12. Write the equilibrium expression for the following chemical reaction;
Keq = [CH4] [H2S]2
[H2]4 [CS2]
Write the equilibrium expression for
the following chemical reaction;
4H2(g) + CS2(g)  CH4(g) + 2H2S(g)
3,2

13. Entropy (S) and Enthalpy (H)
Which two factors together determine
if a reaction is spontaneous or not?
3,3

14. What effect will the addition of KClO4 have on the following
No effect, Keq = [O2]2
What effect will the addition of
KClO4 have on the following
Equilibrium?
KClO4(s)  KCl(s) + 2O2(g)
3,4

15. the rate of a chemical reaction?
Molarity / time
What is the unit usually used to express
the rate of a chemical reaction?
4,1

16. Write the solubility product expression, Ksp, for the dissolution of
Ksp = [Pb+4] [CO3-2]2
Write the solubility product expression,
Ksp, for the dissolution of
lead (IV) carbonate.
4,2

17. It may or may not be spontaneous.
If the entropy and enthalpy
of a chemical reaction both decrease,
what can you conclude about the
spontaneity of the reaction?
4,3

18. left Reducing the temperature on the following
reaction will cause it to shift in which
direction?
N2(g) + 3H2(g) + Energy  2NH3(g)
4,4

19. Write the rate law for the following
Rate = k [N2] [H2]3
Write the rate law for the following
chemical reaction;
N2(g) + 3H2(g)  2NH3(g)
5,1

20. What will the addition of NaCl do To a saturated solution of PbCl2?
The addition of Cl- would cause PbCl2 to precipitate.
What will the addition of NaCl do
To a saturated solution of PbCl2?
5,2

21. The following chemical reaction (will / will not) be spontaneous.
C3H8(g) + 5O2(g)  3CO2(g) + 4H2O(g) + Energy
5,3

22. What effect would adding water to the following reaction have on its
No effect
What effect would adding water to
the following reaction have on its
equilibrium position?
Na(s) + 2H2O(l)  2NaOH(aq) + H2(g)
5,4

23. Final Jeopardy
What is the concentration of carbonate ions in a saturated solution of SrCO3?
Ksp = 9.3 x 10-10