Equilibrium Questions
Which of the following correctly describes the equilibrium constant for the gas-phase reaction between H
2
and O
2
to form gaseous H
2
O : 2H
2(g)
+ O
2(g)
--> 2H
2
0
(g)
K
c
= [H
2
0] / [H
2
][O
2
]
K
c
= [H
2
O]
2
/ [H
2
][O
2
]
K
c
= [H
2
O]
2
/ [H
2
]
2
[O
2
]
K
c
= [H
2
][O
2
] / [H
2
O]
K
c
= [H
2
O]
Consider the quilibrium N
2(g)
+ 3 H
2(g)
-><- 2 NH
3(g)
at a certain temperature. An equilibrium mixture in a 4.00 liter vessel contains 1.60 moles NH
3
, 0.800 moles N
2
, and 1.20 moles H
2
. What is the value of K
c
?
9.00
29.6
3.37
17.1
7.41
An equilibrium mixture is analyzed and found to contain 0.62M N
2
, 0.50M H
2
, and 0.24M NH
3
. What is K
c
for the reaction, N
2(g)
+ 3H
2(g)
<--> 2NH
3(g)
0.74
2.7
1.3
0.60
0.37
At a given temperature, an equilibrium mixture of the reaction 2NO
(g)
+ O
2(g)
<--> 2NO
2(g)
contains 0.090 moles NO, 0.120 moles of O
2
, and 0.060 moles of NO
2
in a 3.00 liter container. The value of K
c
is
3.7
6.1
9.3
11
17
The following system is at equilibrium. In which direction (right or left) will the equilibrium position shift with the following changes?
3NO
(g)
<--> N
2
O
(g)
+ NO
2(g)
+ 154.9 kJ
Lowering the temperature?
Right
Left
No effect
Raising the temperature?
Right
Left
No effect
Adding more N
2
O?
Right
Left
No effect
Adding more NO?
Right
Left
No effect
Removing some N
2
O?
Right
Left
No effect
Adding a catalyst?
Right
Left
No effect
Inreasing the volume?
Right
Left
No effect
Answers