Kp

Question 1

What is partial pressure?

Answer 1

Each gas’s contribution to the total pressure

Question 2

How would you calculate the partial pressure of a gas?

Answer 2

total pressure x moles of gas/total moles

Question 3

What is the mole fraction equation?

Answer 3

Mole fraction of gas A = number of moles of gas A in the mixture ➗ total number of moles of gas in the mixture

Question 4

How do you calculate the units for Kp?

Answer 4

Write out the units for the partial pressures in the same arrangement as the Kp equation and cancel out/multiply together.
Usually in Pa, kPa, atm etc. DO NOT CHANGE UNITS

Question 5

What is the effect of increasing temperature on Kp for an endothermic reaction?

Answer 5

Equilibrium shifts to the right, so partial pressures of products increase, so Kp increases

Question 6

What will be the kinetic effect of increasing the

temperature and pressure for any reaction?

Answer 6

Increasing both will increase the rate of reaction as:
Temperature - many more particles have energy greater than
or equal to the activation energy → more successful collisions per second
Pressure - more particles in the same volume → more
successful collisions per second.