How do I calculate the mass of a product at equilibrium given initial reactant masses and Kp? I really don't mean to abuse this forum
, but I am just stuck So here is the question
Hydrogen can be extracted from natural gas according to the following reaction:
at 825 K
An 85.0 L reaction container initially contains 22.3 kg of CH4
and 55.4 kg of CO2
at 825 K.
Assuming ideal gas behavior, calculate the mass of H2
(in g) present in the reaction mixture at equilibrium.And here is what I did
(I got 16.35M and 14.81M with the moles (found with masses) and 85L)
Assume ideal behavior
Equilibrium concentration of H2 = 2x = 2(1.485) = 2.97M
And then I am stuck.
So I tried doing it as if it wasn't an equilibrium:
1259 mol CO2*2*2.016g H2 = 5.076 kg
But then that just doesn't make sense.
Where should I go from here? Can somebody give me a hint? Please?