Question

Methanol, a potential replacement for gasoline as an automotive fuel, can be made from H2 and CO by the reaction

CO(g) + 2H2(g) CH3OH(g)
At 500.0 K, this reaction has Kp = 6.25 x 10-3. Calculate ?

Answer 1

`\Delta G=-48.2kJ/mol`

Step-by-step explanation:

Hello,

In this case, considering that the relationship between Kp and K is:

`K=(Kp)/(RT^(\Delta \\u))`

Whereas the change in the number of moles (stoichiometric coefficients) is:

`\Delta \\u=1-2-1=-2`

The equilibrium constant is:

`K=(6.25x10^(-3))/((8.314(J)/(mol* K)*500.0K)^(-2))\\\\K=1.08x10^(5)`

In such a way, the Gibbs free energy of reaction is:

`\Delta G=-RTln(K)=-8.314(J)/(mol* K)*500.0K*ln(1.08x10^5)\\\\\Delta G=-48.2kJ/mol`

Regards.