Standard Cell Potential of Daniell Cell

In an electrochemical cell, oxidation and reduction reactions take place simultaneously. When zinc is used as the anode and copper(II) sulfate is the cathode in a Daniell cell, the following two half-reactions occur:

Anode: Zn(s) → Zn²⁺(aq) + 2e^-

Cathode: Cu²⁺(aq) + 2e^- → Cu(s)

Given that the standard electrode potentials (E°) for these half-reactions are +0.34 V for the copper half-reaction and -0.76 V for the zinc half-reaction, calculate the standard cell potential (E°_cell) for the Daniell cell. Which of the following statements is true regarding this cell potential?