# Immersing copper and zinc in hydrochloric acid

I am wondering what would happen if a metal strip of copper and a metal strip of zinc were immersed in solution of $\ce{HCl}$ in standard electrochemical conditions. I have calculated the standard change in Gibb's free energy $\Delta_\mathrm rG^0$ using the relation $\Delta_\mathrm rG^0=-zF\Delta E^0$ where $z$ is the number of electrons exchanged, $F$ is faraday's constant, and $\Delta E^0$ is the standard change in electrode potential. I have found the following values:

$$\Delta_\mathrm rG^0_{\ce{Zn}}=-147\ \mathrm{kJ/mol}, \Delta_\mathrm rG^0_{\ce{Cu}}=-66\ \mathrm{kJ/mol}$$

It appears that the reaction between $\ce{Zn}$ and $\ce{H+}$ is more spontaneous. Does this mean that the reaction with $\ce{Cu}$ will not take place at all?

• Enthalpy or free energy? These are two different things. Make up your mind. – Ivan Neretin Jun 8 '16 at 17:46