Which describes the relationship between Kc and Kp for the reaction?

Question

Equilibrium reaction: N2O4(g) <==> 2NO2(g)

A.) Kp = Kc

B.) Kp = RT x Kc

C.) Kp = (RT x Kc)^-1

D.) Kp = Kc/RT

E.) Kp = RT/Kc

Answer 1

The relationship between Kc and Kp is found in this equation

Kp = Kc * (RT)^deltaN

N is the difference in the amount of moles of reactants and products

Rate is 0.08206 Latm/molK

Temperature is in K

But you don&#039; thave to know all that

The difference between your reactants and products is 1

so Kp = Kc * RT

Answer 2

Kc &#039;s have [Molarities]

to change Molarities into pressures , we use PV=nRT,.,..

re-arranged , it gives Pressure = n/V (RT),...

which says Pressures = Molarities (RT)

so we change Kc = [M] / [M] [M]  into Kp

by [M (RT)] / [M (RT)] [M (RT)]

most of the RT&#039;s cancel out except for one as a denominator

so , this time Kp = Kc / RT

your answer is: D.) Kp = Kc/RT