the equilibrium constant (physical)

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

a reaction is represented by aA(g) + bB(g) <-> cC(g) + dD(g), what Kp for the system?

Answer 4

Kp = pCc pDd / pAa pBb
where pA = partial pressure of A and a = number of moles of A

Question 5

How do you calculate the units for Kp

Answer 5

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 6

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

Answer 6

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

Question 7

what will the kinetic effect of increasing the temperature and pressure for any reaction

Answer 7

increasing both will increase the rate of reaction because:
temperature as many more particles have energy greater or equal to the activation energy so there are more successful collisions.
pressure has more particles in the same volume so more successful collisions happen per second