1. 1. If 6. 00 moles CO2, and 6. 00 moles H2 are put in a 2
1. If 6.00 moles CO2, and 6.00 moles H2 are put in a 2.00 L container at 670 oC, calculate all equilibrium concentrations.
CO(g) H2O(g) ⇄ CO2(g) + H2(g) Keq = 9.0
I M M
C +x +x -x -x
E x x x x
[CO2][H2]
= 9.0
Keq =
[CO][H2O]
Goes left to equilibrium

2. (3 - x)2
Keq =
= 9 x2
Square root both sides
3 - x = 3
x 1
3x = x
4x = 3
[CO] = [H2O] = x = 0.75 M
[CO2] = [H2] = = M

3. 1. The system described by the reaction below is in equilibrium
1. The system described by the reaction below is in equilibrium. [N2O4] is increased. Describe the sequence of changes in the forward and reverse reaction rates until a new equilibrium is attained.
N2O4(g) ⇌ 2NO2(g)

4. 1. The system described by the reaction below is in equilibrium
1. The system described by the reaction below is in equilibrium. [N2O4] is increased. Describe the sequence of changes in the forward and reverse reaction rates until a new equilibrium is attained.
N2O4(g) ⇌ 2NO2(g)

5. 1. The system described by the reaction below is in equilibrium
1. The system described by the reaction below is in equilibrium. [N2O4] is increased. Describe the sequence of changes in the forward and reverse reaction rates until a new equilibrium is attained.
N2O4(g) ⇌ 2NO2(g)

6. Forward Rate Reverse RateI
increases
no change C
decreases
increased E
increases
increased

7. 2. [NO2] is decreased. Describe the sequence of changes in the
2. [NO2] is decreased. Describe the sequence of changes in the forward and reverse reaction rates until a new equilibrium is attained.
N2O4(g) ⇌ NO2(g)
Forward Rate Reverse Rate I
no change
decrease C
decreases
increases E
decreases
decreases

8. 3. Temperature is increased
3. Temperature is increased. Describe the sequence of changes in the forward and reverse reaction rates until a new equilibrium is attained.
Energy N2O4(g) ⇌ 2NO2(g)
Forward Rate Reverse Rate I
increase
by more
increase C
decreases
increases E
increases
increases