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The two methods for the synthesis of methanol are given below. CO(g) + 2H2(g) ⇌ CH3OH(g)...

The two methods for the synthesis of methanol are given below.
CO(g) + 2H2(g) ⇌ CH3OH(g) (1)
CO2(g) + 3H2(g) ⇌ CH3OH(g) + H2O(g) (2)

(a) At 1 atm pressure and 250°C, for the synthesis of methanol from carbon
monoxide the partial pressure of CO:H2:CH3OH are
0.449:0.55075:0.00025 respectively.

Calculate the equilibrium constant for this reaction. Use this value for the
equilibrium constant to calculate the change in the Gibbs Free Energy for
the synthesis of methanol and comment on the sign.

Solutions

Expert Solution

The sign of change in Gibb's free energy is positive. It means that the reaction is not spontaneous in forward direction. Instead the reaction will proceed in backward direction.

If the sign would be negative, then the reaction would proceed in forward direction.

And if the value is zero then the reaction is at equilibrium already.

Also the value of R , chosen is in L atm/ mol• K because while calculating the value of equilibrium constant, we used partial pressure in the units of atm.

Amanda K answered 6 months ago
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