Chemistry, The Central Science, 11th edition
Theodore L. Brown; H. Eugene LeMay, Jr.;
Bruce E. Bursten and Catherine J. Murphy
Chapter 15
Chemical Equilibrium
Donna Narsavage Heald
Siena College
Loudonville, NY
 2009, Prentice-Hall
What is Kp in terms of Kc for the following
reaction ?
2 NO(g) +
1.
2.
3.
4.
5.
Kp = KcRT
Kp = Kc/RT
Kp = KcR/T
Kp = Kc
Kp = Kc/(RT)2
O2(g)
2 NO2(g)
What is Kp in terms of Kc for the following
reaction ?
2 NO(g) +
1.
2.
3.
4.
5.
Kp = KcRT
Kp = Kc/RT
Kp = KcR/T
Kp = Kc
Kp = Kc/(RT)2
O2(g)
2 NO2(g)
What is the correct equilibrium constant
expression for the reaction:
P4(s)
+
6 Cl2(g)
4 PCl3(l)
What is the correct equilibrium constant
expression for the reaction:
P4(s)
+
6 Cl2(g)
4 PCl3(l)
Which accurately reflects the changes in concentration
that will occur if O2 is added to disturb the equilibrium?
2 NO(g)
+
O2(g)
2 NO2(g)
[NO]
[O2]
[NO]
1.
Increase
Increase
Increase
2.
Increase
Increase
Decrease
3.
Decrease
Decrease
Decrease
4.
Decrease
Decrease
Increase
5.
Decrease
Increase
Increase
Which accurately reflects the changes in concentration
that will occur if O2 is added to disturb the equilibrium?
2 NO(g)
+
O2(g)
2 NO2(g)
[NO]
[O2]
[NO]
1.
Increase
Increase
Increase
2.
Increase
Increase
Decrease
3.
Decrease
Decrease
Decrease
4.
Decrease
Decrease
Increase
5.
Decrease
Increase
Increase
Which of the following will result in an
equilibrium shift to the right?
PCl3(g) + Cl2(g)
1.
2.
3.
4.
5.
PCl5(g)
DH° = –87.9 kJ/mol
Increase temperature/increase volume
Increase temperature/decrease volume
Decrease temperature/increase volume
Decrease temperature/decrease volume
None of the above
PCl5
Which of the following will result in an
equilibrium shift to the right?
PCl3(g) + Cl2(g)
1.
2.
3.
4.
5.
PCl5(g)
DH° = –87.9 kJ/mol
Increase temperature/increase volume
Increase temperature/decrease volume
Decrease temperature/increase volume
Decrease temperature/decrease volume
None of the above
PCl5
What is the value of Kc for the reaction?
2 CO(g) + O2 (g)
CO2(g)
1.
2.
3.
4.
5.
2CO2(g)
CO(g) + 1/2 O2(g)
Kc = 1/(5.0 x 1018)1/2
Kc = 1/(2.5 x 1018)
Kc = –(5.0 x 1018)/2
Kc = –(5.0 x 1018)1/2
Kc = 2/(5.0 x 1018)1/2
Kc = 5.0 x 1018 at 25 °C
Kc = ??
at 25 °C
What is the value of Kc for the reaction?
2 CO(g) + O2(g)
CO2(g)
1.
2.
3.
4.
5.
2 CO2(g)
CO(g) + 1/2 O2(g)
Kc = 1/(5.0 x 1018)1/2
Kc = 1/(2.5 x 1018)
Kc = –(5.0 x 1018)/2
Kc = –(5.0 x 1018)1/2
Kc = 2/(5.0 x 1018)1/2
Kc = 5.0 x 1018 at 25 °C
Kc = ??
at 25 °C