# Equilibrium Concentration Homework

```Equilibrium Concentration Homework
1)
The reaction ____ N2 + ____ O2  ____ NO has an equilibrium constant
of 9.7 x 10-29 at 3230 C. If the equilibrium partial pressure of N2 is 0.50
atm and the equilibrium partial pressure of O2 is 0.40 atm, what will the
equilibrium pressure of NO be? Is this reaction a good one for making
NO? Explain.
2)
When the reaction above is performed at 2400 K, the equilibrium constant
for the reaction is 0.0025. If the equilibrium partial pressures are the same
as in problem 1, what is the equilibrium partial pressure of NO? Is this
reaction a good one for making NO? Explain.
3)
When I performed the equilibrium ____ NO + ____ O2  ____ NO2 at 450
K, I found that the equilibrium constant was 14,625. If the equilibrium
partial pressure of NO is 0.10 atm and the equilibrium partial pressure of
O2 is 0.16 atm, what is the equilibrium partial pressure of NO2?
4)
The equilibrium constant for the process A + 2 B  C + 2 D is 0.075.
When I perform this reaction, I found that the equilibrium concentration of
A was 0.20 M, the equilibrium concentration of B was 0.35 M, and the
equilibrium concentration of C was 0.05 M. This reaction will only be
financially feasible if the equilibrium concentration of D is greater than
0.075 M. Using your knowledge of equilibria, should I invest my money
into a factory that performs this reaction?
1)
The reaction 1 N2 + 1 O2  2 NO has an equilibrium constant of 9.7 x 1029 at 3230 C. If the equilibrium partial pressure of N is 0.50 atm and the
2
equilibrium partial pressure of O2 is 0.40 atm, what will the equilibrium
pressure of NO be? Is this reaction a good one for making NO? Explain.
PNO = 4.4 x 10-15 atm, probably not.
2)
When the reaction above is performed at 2400 K, the equilibrium constant
for the reaction is 0.0025. If the equilibrium partial pressures are the same
as in problem 1, what is the equilibrium partial pressure of NO? Is this
reaction a good one for making NO? Explain.
PNO = 0.022 atm, still probably not.
3)
When I performed the equilibrium 2 NO + 1 O2  2 NO2 at 450 K, I found
that the equilibrium constant was 14,625. If the equilibrium partial
pressure of NO is 0.10 atm and the equilibrium partial pressure of O2 is
0.16 atm, what is the equilibrium partial pressure of NO2?
4.84 atm
4)
The equilibrium constant for the process A + 2 B  C + 2 D is 0.075.
When I perform this reaction, I found that the equilibrium concentration of
A was 0.20 M, the equilibrium concentration of B was 0.35 M, and the
equilibrium concentration of C was 0.05 M. This reaction will only be
financially feasible if the equilibrium concentration of D is greater than
0.075 M. Using your knowledge of equilibria, should I invest my money
into a factory that performs this reaction?
[D] = 0.192 M; Yes, invest away!
```