[3.1.10] Equilibrium Constant Kₚ for Homogeneous Systems Flashcards
1
Q
How do you calculate the partial pressure of a gas?
A
- Partial pressure = mole fraction x total pressure
2
Q
How do you calculate a mole fraction for a gas?
A
- Mole fraction = number of moles of a gas / total number of moles of all gases
- e.g. For a 3-part mixture:
- x₁ = y₁ / y₁ + y₂ + y₃
3
Q
A
4
Q
What state of matter do Kp expressions only contain?
A
- Gaseous.
- Any substance in another state is left out.
5
Q
Write an expression for Kp using this equation:
A
6
Q
In the equation below, Kp is measured in kPa. Deduce the units of Kp.
A
7
Q
A
8
Q
What conditions affect the value of Kp?
A
- Kp only changes with temperature.
- It does not change if pressure or concentration are altered or if there is a catalyst present.
9
Q
What does the size of the Kp value indicate?
A
- The larger the Kp value, the greater the amount of products.
- If Kp is small, we say the equilibrium favours the reactants.
10
Q
Describe the effect of temperature on the position of equilibrium and Kp.
A
- Both the position of equilibrium and Kp will change if the temperature is altered.
11
Q
Describe what would happen to the equilibrium and Kp if the temperature was increased in the reaction below.
A
12
Q
Describe the effect of pressure on the position of equilibrium and Kp.
A
- The position of equilibrium will change if pressure is altered but the value of Kp stays constant as Kp only varies with temperature.
13
Q
Describe what would happen to the equilibrium and Kp if the pressure was increased in the reaction below.
A
