What are the values of Kc and Kp of this reaction?

Question

At equilibrium, a sample of gas from the system is collected into a 5.00L flask. It is found to contain 8.62 grams of CO, 2.60 g of H2, 43.0 g of CH4, and 48.4 g of H2O (Note all of these are in gaseous form) at 320 degrees C.

CH4(g) + H20(g) <> CO(g) +3H2(g)

Answer 1

Kc = [CO] [H2]³ / [CH4] [H2O]. [ ] are the concentrations of each gas in moles/L

[CO] = 8.62 g / 28.0 g/mole / 5L = 0.0616 M

[H2] = 2.60 g /2.02g/mole / 5L = 0.257 M

[CH4] = 43.0 g / 16.0 g /mole / 5L = 0.538 M

[H2O] = 48.4 g / 18.0 g/mole / 5L = 0.538 M

Kc = 0.0616 x 0.257³ / 0.538 x 0.538 = 0.00361

Kp = Kc x (RT)^Δn where Δn = moles gaseous products - moles gaseous reactants = 2 , R is gas constant 0.0821 L-atm/mole-deg, and T is absolute temperature 593 K.

Kp = 0.00361 x (0.0821 x 593)² = 8.56

Please check math.