not really, no. There is a relationship between the cell potential and the gibbs free energy, though:
[math]\Delta G = -nFE[/math]
where [math\Delta G[math] is the gibbs free energy, n is the number of moles of electrons involved in the process, F is the Faraday constant (the charge on a mole of electrons, so that "nF" is equal to the charge used), and E is the voltage required or provided (depending on whether the process is spontaneous or not). In reality, though, the calculated value of E and the real value of E are usually different, due to a phenomenon known as overpotential, which is more prevalent when gases are involved.
In general, if [math]\Delta G[/math] is negative, E will be positive, meaning the process is spontaneous, and that electricity will be generated, and if the reverse is true, the process will require energy input for it to occur. The latter situation is often an electrolysis.