Electrochemical Cell Potential Calculation

In electrochemistry, the Nernst equation relates the electromotive force (EMF) of a cell to the concentrations of the reactants and products involved in the electrochemical reaction. Consider a galvanic cell that uses the following half-reactions at 25°C:

Oxidation: Zn(s) → Zn²⁺(aq) + 2e^-
Reduction: Cu²⁺(aq) + 2e^- → Cu(s)

Given that the standard reduction potentials for these half-reactions are: E_°(Zn²⁺/Zn) = -0.76 V and E_°(Cu²⁺/Cu) = +0.34 V, calculate the standard cell potential (E_cell^°) for this galvanic cell and determine which of the following statements regarding the cell potential at non-standard conditions (where [Zn²⁺] = 0.10 M and [Cu²⁺] = 1.0 M) is correct.