equilibrium 2 p1

Question 1

partial pressure

Answer 1

each gas’s contribution to the total pressure
partial pressure p = mole fraction x total pressure

Question 2

mole fraction

Answer 2

moles of gas / total number of moles of gas in the mixture

Question 3

what does a Kp equation look like?

Answer 3

pCc x pDd/pAa x pBb
pA = partial pressure of A and a = number of moles of A
units - work out for each reaction using the units given e.g. Pa, atm, etc

Question 4

how does increased temperature of an endothermic reaction effect Kp?

Answer 4

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

Question 5

how does decreased temp of an endothermic reaction effect Kp?

Answer 5

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

Question 6

how does pressure affect the value of Kp?

Answer 6

it doesn’t

Question 7

how does increased temp or pressure affect any reaction?

Answer 7

temp - 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