Cell Potential of a Galvanic Cell

In electrochemistry, galvanic cells are devices that convert chemical energy into electrical energy through spontaneous redox reactions. In this context, consider a galvanic cell composed of a zinc electrode immersed in a zinc sulfate solution and a copper electrode immersed in a copper sulfate solution. The standard reduction potentials for the half-reactions are as follows: Zn²⁺ + 2e^- → Zn (s) (E^° = -0.76 V) and Cu²⁺ + 2e^- → Cu (s) (E^° = +0.34 V). What is the overall cell potential (E^cell) for this galvanic cell?