Kp

Question 1

What is the expression for the equilibrium constant, Kp? (4)

Answer 1

The equilibrium constant for this reaction is:

p(a)^a x p(b)^b

Where P represents the partial pressure, and a, b, c and d are the number of
moles of the species A, B, C and D which appear in the balanced equation for
the equilibrium.

Question 2

How do you calc mole fraction

Answer 2

Mole fraction=Moles/Total moles

Question 3

How do you calculate partial pressures of gas? (3)

Answer 3

Partial pressure=mole fraction x total pressure

Question 4

What is the only factor that affects Kp? (1)

Answer 4

Temperature

Question 5

Summary diagram to show effects of changes in temperature on Kp (12)

Answer 5

ΔΗ, Forward reaction, Change in temperature, Shift in eqm. position, eqm. Yield of product, Equilibrium constant K

-ve, exothermic, increase, left ,decrease, decrease

-ve, exothermic, decrease ,right ,increase ,increase

+ve ,endothermic ,increase ,right ,increase ,increase

+ve, endothermic, decrease, left ,decrease ,decrease

Question 6

Summary diagram to show effects of changes in pressure on Kp (6)

Answer 6

Increase in pressure= eqm pos shifts to the right and yield of product increases No effect to Kp

Decrease in pressure= eqm pos shifts to the left and yield of product decreases No effect to Kp

Question 7

Summary diagram to show effects of catalysts on Kp (4)

Answer 7

Just has no affect overall

Question 8

Use curly brackets not square brackets for KP

Answer 8

gjf

Question 9

Units for kP

Answer 9

kPA1
would be kPA-1 if on the denominator

Question 10

DINT FORGET TO ADD P ON THE BRACKEWTS

Answer 10

vvf

Question 11

How do you reafrrange to find the total prrssure of a reaction

Answer 11

reactants x kP / products

Question 12

Work out the units

Answer 12

kPa2/ kPa kPa3

kPa-2

Question 13

Ensure you do not use square brackets

Answer 13

dfa

Question 14

In this equilibrium which is exothermic in the forward direction
N2+ 3H2<–> 2 NH3
If temperature is increased what happens

Answer 14

the reaction will shift to oppose the change
and move in the backwards endothermic direction. The position of
equilibrium shifts left. The value of Kp gets smaller as there are fewer
products.