Consider the following chemical equilibrium:
C(s) + 2H2 (g) <> CH4 (g)
Now write an equation below that shows how to calculate Kp from Kc for this reaction at an absolute temperature T. You can assume T is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator.

Kp = [CH₄(g)]/[H₂(g)]²(RT)⁻¹

Explanation:

C(s) + 2H₂(g) => CH₄(g)

Kp = Kc(RT)ⁿ

n= change in molar volumes of gas = 1 - 2 = -1

R = 0.08206 L·Atm/mol·K (gas constant)

T = Kelvin Temperature (arbitrary in problem) K =°C + 273

Kc = [CH₄(g)]/[H₂(g)]²  (measured values need to be in moles/L)

Kp = [CH₄(g)]/[H₂(g)]²(RT)⁻¹

8 carbon atoms forming single bonds with 18 hydrogen atoms; a triple bond exists between the third and fourth carbon atom from the right

explanation: