Question

For the following reaction at equilibrium in a closed vessel, ΔrH = −153 kJ per mol of CH3CHO.
CH3CHO(g) ⇌ CH4(g) + CO(g)

Which of the following statements are correct?

a. For the thermodynamic equilibrium constant, K at 298 K is greater than K at 500 K.
b. At 25 oC, K = Kp
c. Adding a catalyst will not affect the equilibrium partial pressure of CO(g).
d. Adding some CH4(g) will decrease the equilibrium partial pressure of CH3CHO(g).
e. Decreasing the volume of the system will decrease the moles of CO(g) at equilibrium.
f. At 25 oC, Kp < Kc

Answer 1

no idea how to do this

Answer 2

is it b and d?

Answer 3

Why do you believe b and d are correct?
All of these are Le Chatelier's Principle. You should know that b can't be right.. You know that Kp = Kc*RT)^delta n so the only time Kp can equal Kc is when delta n is zero. In this reaction you have 2 mols products and 1 mol reactant so delta n isn't zero. It's 1.