E-2 Quantitative Equilibrium Flashcards
Don’t use a calculator!
2 A (g) + B (g) ⇔ A2B (g) + heat
The Kp for the above reaction is 10. What is the K’p for the following reaction?
A2B (g) + heat⇔2 A (g) + B (g)
K’p = 1/10 = 0.1
Don’t use a calculator!
2 M (s) + N (g) ⇔ M2N (g) + heat
The Kp for the above reaction is 0.01. What is the K’p for the following reaction?
M2N (g) + heat⇔2 M (s) + N (g)
K’p = 1/Kp = 100
Don’t use a calculator!
2 A (g) + B (g) ⇔ A2B (g) + heat
The Kp for the above reaction is 10. What is the K’p for the following reaction?
4 A (g) + 2 B (g) ⇔ 2 A2B (g) + heat
Reaction is doubled so K value is squared; K’p = Kp2 = 100
Don’t use a calculator!
X2 (g) + Y2 (g) + heat ⇔ 2 XY (g)
The Kp for the above reaction is 9. What is the K’p for the following reaction?
1/2 X2 (g) + 1/2 Y2 (g) + heat ⇔ XY (g)
Reaction is halved so K value is squared root; K’p = Kp1/2 = 3
2 A (g) + B (g) ⇔ A2B (g) + heat
What is the change in n for the gases in this reaction?
nproducts - nreactants = -2
X2 (g) + Y2 (g) + heat ⇔ 2 XY (g)
What is the change in n for the gases in this reaction?
nproducts - nreactants = 0
2 M (s) + N (s) ⇔ M2N (g) + heat
What is the change in n for the gases in this reaction?
nproducts - nreactants = 1; M and N are both solids
You will need a calculator!
2 A (g) + B (g) ⇔ A2B (g) + heat
The value for Kc for this reaction is 700 when the temperature is 27 °C. What is the value for Kp?
Kp = 1.15
You will need a calculator!
X2 (g) + Y2 (g) + heat ⇔ 2 XY (g)
The value for Kp for this reaction is 10 when the temperature is 27 °C. What is the value for Kc?
Kc = 10
You will need a calculator!
2 M (s) + N (s) ⇔ M2N (g) + heat
The value for Kp for this reaction is 0.050 when the temperature is 27 °C. What is the value for Kc?
Kc = 0.0020
Right, Left, or No Impact
2 A (g) + B (g) ⇔ A2B (g) + heat
The above reaction has a Kp = 10. Which way will the reaction shift if the current partial pressures of all substances is 1 atm?
right
Right, Left, or No Impact
X2 (g) + Y2 (g) + heat ⇔ 2 XY (g)
The above reaction has a Kp = 0.10. Which way will the reaction shift if the current partial pressures of all substances is 1 atm?
left
2 M (s) + N (s) ⇔ M2N (g) + heat
The solids M and N are combined in an empty flask. Several minutes later the partial pressure of M2N is 0.15 atm and the masses of 1.5 grams and 0.50 grams, respectively. What is the value for Kp?
Kp = PM2N = 0.15 since both M and N are solids.
2 A (g) + B (g) ⇔ A2B (g) + heat
The gases A (1.0 atm) and B (1.0 atm) are combined in an empty flask. At equilibrium, the partial pressures of A, B , and A2B are 0.50, 0.75, and 0.25 atm, repectively. What is the value for Kp?
Kp = 1.3
X2 (g) + Y2 (g) + heat ⇔ 2 XY (g)
An empty 1.0 L flask is filled with 1.0 moles of X2 and 1.0 moles of Y2. At equilibrium, the concentrations are 0.80 M for X2, 0.80M for Y2 and 0.40M for XY. What is the value for Kc?
Kc = 0.25
