[yankeekd25]

Consider the reaction

H2(g) + C2H4(g) --> C2H6(g)

Using the standard thermodynamic data in the tables linked above, calculate deltaG for this reaction at 298.15K if the pressure of each gas is 26.89 mm Hg.

delta G for C2H6(g)= -32.8
          for C2H4(g)= 68.2
          for H2 (g)  =  0

What effect does the pressure have the Gibbs free energy calculations?

[leve]

What can you use the given pressures to calculate?

There are a few equations using deltaG. Which one would you use pressure for?

[yankeekd25]

What can you use the given pressures to calculate?

There are a few equations using deltaG. Which one would you use pressure for?

Can you use the pressures to find Kp, then use the equilibrium constant, then plug it into the

G= -RT ln k?

[joshuaeddy27]

you might try this
(delta)G = (delta)G(std) + RTln(Q)

the delta G changes in relation to the temperature and you can use the partial pressures to figure out the Q.  it doesn't seem like the entire question was posted.