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...
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 cell?
Answer Details
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).