This question is from Chemisry Chang, 12th ed, P 630
Methanol (CH3OH) is manufactured industrially by the reaction
CO(g) ..> 2H2(g) + CH3OH(g)
The equilibrium constant (Kc) for the reaction is 10.5 at 220°C. What is the value of KP
at this temperature?
The answer is Kp = 6.41 E-3
How is that Kc indicates that the equilibrium favors the products, while Kp favors the reactants. and How does is that DG has afferent signs in these two cases?
Any ideas?
The reaction
CO(g) ..> 2H2(g) + CH3OH(g)
should be written as
CO(g) + 2H2(g) = CH3OH(g)
Ismail Badran
Check the calculations of the equilibrium constants.
The equilibrium constant calculated from partial pressures is equal to the concentration equilibrium constant calculated in moles multiplied by RT to the power △ n. Where △n = (c+ d) – (a+b), i.e. The number of moles of gaseous products minus the number of moles of gaseous reactants in a balanced chemical reaction.
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