equilibrium II

Question 1

what is partial pressure

Answer 1

the pressure an individual gas exerts

Question 2

what is the total pressure

Answer 2

sum of all the partial pressure of the individual gases

Question 3

what is a mole fraction

Answer 3

portion of a gas mixture that is a particular gas

Question 4

mole fraction of gas in a mixture equation

Answer 4

mole fraction of gas in a mixture= number of moles / total number of moles of gas in the mixture

Question 5

partial pressure of a gas equation

Answer 5

partial pressure of gas = mole fraction x total pressure of the mixture

Question 6

What is Kp and how is it different from Kc?

Answer 6

Kp is an equilibrium constant used for equilibria involving gases. Its expression is similar to Kc, but instead of concentrations, it deals with partial pressures of gases.

Question 7

What is the expression for the equilibrium constant
Kp for the reaction
aA+bB⇌dD+eE involving gases?

Answer 7

K = p(D)^dp(E)^e(g)/p(A)^ap(B)^b

Question 8

When writing an expression for Kp for a heterogeneous equilibrium, what components should be included?

Answer 8

Only include gases in the expression

Question 9

How do changes in concentration, pressure, and temperature affect equilibrium constants kc and kp

Answer 9

Concentration and pressure changes do not affect the values of kc and kp
. They alter the amounts of products and reactants at equilibrium, but the ratio remains constant.
Temperature changes affect both the amounts of products and reactants at equilibrium and the values of the equilibrium constants.

Question 10

What effect do catalysts have on the position of equilibrium and the values of Kc and Kp

Answer 10

Catalysts have no effect on the position of equilibrium or the value of Kc and Kp
They cannot increase yield, but they do accelerate the approach to equilibrium.