1/04/25 Test

Question 1

Define total pressure.

Answer 1

the total pressure in a reaction is the sum of all the pressures the individual gases (partial pressure)

Question 2

what brackets do we use for Kp?

Answer 2

( )

Question 3

what is a mole fraction?

Answer 3

the proportion (fraction) of a gas in a gas mixture

Question 4

equation for mole fraction

Answer 4

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

Question 5

equation for partial pressure

Answer 5

mole fraction of gas x total pressure in mixture

Question 6

how to calculate Kp

Answer 6

partial pressure of products/ partial pressure of reactants e.g. aA + bB ⇌ cC + dD
= (pC)^c (pD)^d / (pA)^a (pB)^b

Question 7

What affects Kp?

Answer 7

• ONLY temp. changes
• if equilibria shifts in endothermic direction = Kp decreases
• if equilibria shifts in exothermic direction = Kp increases

Question 8

write a general expression for the partial pressure of a gas in a mixture of gases in terms of total pressure

Answer 8

p = total pressure x mole fraction