determine the Kc and mass of product obtained!! 1. The problem statement, all variables and given/known data Consider a chemical reaction CO (g) + 2H2 (g) <-> CH3OH(g). When 2 moles of CO were reacting with 4 moles of H2 at temperature 500K and pressure p = 100bar, and chemical equilibrium was reached, n = 366.0 moles of CO was consumed. Based on the given data determine the value of the chemical equilibrium constant K(T) for T = 500K and find the mass (m) of the product obtained in the reaction. 2. Relevant equations Kp = Kc (RT)Δn PV = nRT aA + bB <=> cC + dD Kp = [PC]c[PD]d / [PA]a[PB]b Kc = [C]c[D]d /[A]ab 3. The attempt at a solution Okay so here is what I did. First the ice chart CO (g) + 2H2 (g) <-> CH3OH Ini 2mol 4mol - Ch -(.366) -2(.366) +(.366) Eq. 1.364 3.268 0.366 ∴Total Moles = 4.998 mol Eq. mol fraction = (Eq. mol / Total Mol) ∴ CO = 0.273 & H2 = 0.654 & CH3OH = 0.073 Eq. partial pressure = Eq. mol frac X pressure ∴ CO = 26.9 atm & H2 = 64.5 atm & CH3OH = 7.2 atm Kp = [7.2]/([26.9][64.5]2) => 6.43 E -5 ∴ Kc = Kp/(RT)Δn = 0.108 To calculate mass I treated it as ideal gas so PV = nRT Where n = total mol = 4.998mol; T = 500K; P = 100 bar = 98.6 atm; R = 0.082 atm dm3 K-1 mol-1 Total Volume = 2.08 dm3 = 2.08 L Now using density we can find the mass where density is 791.80g/L and d = m/V ∴ m = d x V = 791.80 x 2.08 = 1646.944 g Please let know if this problem was approached in the correct way or not.