Transcript Chapter 18 Jeopardy _Reaction Rates and Equilibrium_

Chapter 18 – Reaction
Rates and Equilibrium
Rates of
Reactions
Equilibrium
Entropy and
Free Energy
Le Chatelier’s
Principle
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Temperature or concentration of reactants
The rate of a chemical reaction
may be increased by increasing
the _______ and / or ________.
Row 1, Col 1
They are equal.
When a reaction reaches equilibrium,
what can you say about the rate of
the forward reaction and reverse
reaction?
1,2
Entropy (S)
What is the name and the symbol of
the term used to describe the
‘disorder’ of a process?
1,3
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
Increase
As the particle size of a reactant
decreases, the rate of reaction
will __________.
2,1
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
Increase
Is there an increase or decrease in
The entropy in the following process?
CaCO3(s)  CaO(s) + CO2(g)
2,3
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
It lowers the activation energy.
How does a catalyst speed up a
chemical reaction?
3,1
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
Entropy (S) and Enthalpy (H)
Which two factors together determine
if a reaction is spontaneous or not?
3,3
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
Molarity / time
What is the unit usually used to express
the rate of a chemical reaction?
4,1
Ksp = [Pb+4] [CO3-2]2
Write the solubility product expression,
Ksp, for the dissolution of
lead (IV) carbonate.
4,2
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
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
Rate = k [N2] [H2]3
Write the rate law for the following
chemical reaction;
N2(g) + 3H2(g)  2NH3(g)
5,1
The addition of Cl- would cause PbCl2 to
precipitate.
What will the addition of NaCl do
To a saturated solution of PbCl2?
5,2
will
The following chemical reaction
(will / will not) be spontaneous.
C3H8(g) + 5O2(g)  3CO2(g) + 4H2O(g) + Energy
5,3
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
Final Jeopardy
• What is the concentration of carbonate
ions in a saturated solution of SrCO3?
Ksp = 9.3 x 10-10