Topic 11- Further Equilibrium

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

partial pressure p= mole fraction x total pressure

Question 3

What is the mole fraction?

Answer 3

mole fraction of gas X= number of moles of gas X in the mixture/ total number of moles of gas in the mixture

Question 4

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

Answer 4

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

Question 5

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

Answer 5

Kp decreases because equilibrium shifts to the left, so partial pressure of reactants increases

Question 6

What effect does increasing the pressure have on the Kc/Kp value?

Answer 6

Pressure doesn’t effect Kp

Question 7

What will be the kinetic energy of increasing the pressure and temperature for any reaction?

Answer 7

increasing both will increase the rate of reaction as:

• temperature, many more particles have greater energy than the activation energy–> more successful collisions per second
• pressure, more particles in the same volume–> more successful collisions per second

Question 8

What is the effect of changing concentration or pressure or by the addition of a catalyst on the equilibrium constant?

Answer 8

There is no effect

Question 9

How do you calculate the mole fraction of a substance?

Answer 9

number of moles of substance/total number of moles of gas