In this worksheet, we will practice converting between equilibrium constants defined by partial pressures and those defined by concentration.

**Q1: **

For the reaction , at . If partial pressures are measured relative to a standard pressure of 1 atm, what is the value of at this temperature?

- A
- B
- C
- D
- E0.122

**Q2: **

For the reaction , at . If partial pressures are measured relative to a standard pressure of 1 atm, what is the value of at this temperature?

- A
- B
- C
- D
- E

**Q3: **

For the reaction , at . If partial pressures are measured relative to a standard pressure of 1 bar, what is the value of at this temperature?

**Q4: **

For the reaction , at . If partial pressures are measured relative to a standard pressure of 1 bar, what is the value at this temperature?

- A0.50
- B
- C
- D
- E

**Q5: **

What is the equation for the conversion of to for the reaction

- A
- B
- C
- D
- E

**Q6: **

What is the equation for the conversion of to for the following reaction?

- A
- B
- C
- D
- E

**Q7: **

What is the equation for the conversion of to for the reaction

- A
- B
- C
- D
- E

**Q8: **

is equal to 0.28 for the following reaction at : Under standard conditions, all species have a concentration of 1.00 M and partial pressure of 1.00 atm. Calculate for this reaction at .

- A
- B
- C
- D
- E0.28

**Q9: **

What is the equation for the conversion of to for the reaction

- A
- B
- C
- D
- E

**Q10: **

What is the equation for the conversion of to for the reaction

- A
- B
- C
- D
- E

**Q11: **

What is the equation for the conversion of to for the reaction

- A
- B
- C
- D
- E

**Q12: **

At , the following reaction has : Under standard conditions, the concentration of each species is 1.00 M and the partial pressure is 1.00 bar. Calculate the value of at for this reaction.