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Calculate the equilibrium constant of the reaction CO(g) + H2(g) ⇌ H2CO(g) given that for the...

Calculate the equilibrium constant of the reaction CO(g) + H2(g) ⇌ H2CO(g) given that for the production of liquid formaldehyde ΔrG< = +28.95 kJ mol−1 at 298 K and that the vapour pressure of formaldehyde is 1500 Torr at that temperature.

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The given reaction is, CO(g)+H2 (8)HCO(s) Given that the Gibbs free energy of liquid formaldehyde is 28.95 kJ/mol at 295 K. The vapor pressure of formaldehyde is 1500 Torr. The equilibrium constant for the given reaction can be calculated from the relation: ơ-the satndard Gibbs free energy of the reaction. R-ideal gas constant. T-standard temperature. K -Equilibrium constant The Gibbs free energy of the reaction is the sum of the Gibbs free energy of the liquid formaldehyde production and free energy for the vaporization of liquid formaldehyde. Δ,G-A,G (H.co (1))-A,apG. (H,CO(1)) A,G (H,CO()), the standard Gibbs free energy change for the formation of formaldehyde liquid phase is given as 28.95 kJ/mol.

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