Electrochemical Reactions and Batteries Quiz

To prevent corrosion by sacrificing the zinc instead of the steel.

One on the anode electrode and one on the cathode electrode.

In volts.

<p>By subtracting the electrode potential of the anode from that of the cathode.</p> Signup and view all the answers

<p>By introducing a different metal that is more easily oxidized than the metal to be protected.</p> Signup and view all the answers

<p>To capture electricity and produce power.</p> Signup and view all the answers

<p>The zinc container.</p> Signup and view all the answers

<p>The carbon rod.</p> Signup and view all the answers

<p>Anode: Zn(s) = Zn2+ (aq) + 2e-, Cathode: 2MnO2 (s) + H2 O (l) + 2e- = Mn2 O3 (s) + 2OH- (aq).</p> Signup and view all the answers

<p>By coating the metal with a more easily oxidized metal, such as zinc, through a process called galvanization.</p> Signup and view all the answers

<p>The two half-reactions in an electrochemical cell are the anode electrode and the cathode electrode.</p> Signup and view all the answers

<p>Oxidation occurs at the anode electrode, causing the loss of electrons.</p> Signup and view all the answers

<p>Reduction occurs at the cathode electrode, causing the gain of electrons.</p> Signup and view all the answers

<p>The full cell reaction can be written by combining both half-reactions. For example, in the case of zinc and copper electrodes, the reaction is written as: $Zn(s) + Cu^{2+}(aq) = Zn^{2+}(aq) + Cu(s)$.</p> Signup and view all the answers

<p>An electrochemical cell diagram is typically shown as: Anode electrode - anode solution - cathode solution - cathode electrode. For example, in the case of zinc and copper electrodes, the diagram is shown as: $Zn(s) - Zn^{2+}(aq) - Cu^{2+}(aq) - Cu(s)$.</p> Signup and view all the answers