3.1.10 Equilibrium constant Kp for homogeneous systems

Question 1

equation for calculating partial pressure

Answer 1

partial pressure=mole fraction of gas x total pressure

Question 2

equation for mole fraction

Answer 2

mole fraction=no. of moles/total no. of moles of all gases

Question 3

what is Kp

Answer 3

equilibrium constant

Question 4

what does the Kp expression only include

Answer 4

gases

Question 5

what does the p mean in Kp

Answer 5

partial pressure of that gas

Question 6

how do you write an expression for Kp

Answer 6

p (products)-to the power of moles
divided by p (reactants) to the power of moles multiplied

Question 7

what effect does a larger Kp value have

Answer 7

greater amount of products

Question 8

if Kp is small, the equilibrium favours the…

Answer 8

reactants

Question 9

what is the only thing that effects Kp or Kc

Answer 9

temperature

Question 10

will a catalyst have any effect on the Kp value

Answer 10

no

Question 11

what is the effect on the Kp value, if the forward reaction is exothermic and the temperature is increased

Answer 11

equilibrium will shift backwards in the endothermic direction
to oppose change
value of Kp gets smaller
as there are fewer products formed

Question 12

in an equilibrium reaction there are fewer moles of gas on the product side, what effect does an increase in pressure on position of equilibrium and the Kp value?

Answer 12

equilibrium shifts to the forward direction, side with fewer moles of gas
to oppose the change in pressure
NO effect on Kp value as only temperature changes it

Question 13

What does the effect of the addition of a catalyst on an equilibrium reaction

Answer 13

No change in Kp
Speeds up rate at which reaction reaches equilibrium