Consider the electrochemical cell represented below Zn(s)/Zn2+(aq)//Cu2+(aq)/Cu(s). Which of the following equations describes the reaction occurring in the...

The electrochemical cell is composed of two half-cells: Zn_(s)/Zn²⁺_(aq) and Cu²⁺_(aq)/Cu_(s). The anode (negative electrode) is the Zn_(s)/Zn²⁺_(aq) half-cell, where oxidation occurs, and the cathode (positive electrode) is the Cu²⁺_(aq)/Cu_(s) half-cell, where reduction occurs. During the oxidation process at the anode, solid zinc (Zn) is oxidized to form Zn²⁺ ions, which are released into the solution. This is represented by the half-equation: Zn_(s) → Zn²⁺_(aq) + 2e^- During the reduction process at the cathode, Cu²⁺ ions in the solution are reduced to form solid copper (Cu). This is represented by the half-equation: Cu²⁺_(aq) + 2e^- → Cu_(s) The overall equation for the cell reaction can be obtained by adding the two half-equations and canceling out the electrons: Zn_(s) + Cu²⁺_(aq) → Zn²⁺_(aq) + Cu_(s) Therefore, the correct equation that describes the reaction occurring in the cell is Zn_(s) + Cu²⁺_(aq) → Zn²⁺_(aq) + Cu_(s). Answer (C).