All of the following statements concerning voltaic cells are true except 1) oxidation occurs at the cathode. 2) a salt bridge allows

Question

All of the following statements concerning voltaic cells are true except: 1) oxidation occurs at the cathode; 2) a salt bridge allows cations and anions to move between the half-cells; 3) electrons flow from the anode to the cathode in the external circuit; 4) a voltaic cell can be used as a source of energy; 5) a voltaic cell consists of two half-cells.

Anonymous · Accepted Answer

oxidation occurs at the cathode.Explanation:In a voltaic cell electrons move from anode to cathode. At the anode, species give up electrons. This is an oxidation reaction depicted by the oxidation half equation. At the cathode, species accept electrons and become reduced. This is depicted by the reduction half equation. In summary; in a Voltaic cell, oxidation occurs at the anode while reduction occurs at the cathode.

Anonymous · Answer

Anode half reaction; Co(s) > Co^2+(aq) + 2eCathode half reaction;2Ag^+(aq) + 2e> 2Ag(s)Explanation:A voltaic cell is an electrochemical cell that spontaneously produces electrical energy from chemical reactions. A voltaic cell comprises of an anode (where oxidation occurs) and a cathode (where reduction occurs). The both electrodes are connected with a wire . A salt bridge ensures charge neutrality in the anode and cathode compartments. Electrons flow from anode to cathode. For the cell referred to in the question;Anode half reaction;Co(s) > Co^2+(aq) + 2eCathode half reaction;2Ag^+(aq) + 2e> 2Ag(s)

Anonymous · Answer

d)Cells 1 and 2Explanation:In a voltaic cell, oxidation occurs at the anode and reduction occurs at the cathode. The half cell that function as anode or cathode in a voltaic cell depends strictly on the reduction potential of the metal ion/metal system in that half cell.Examining the reduction potentials of the various metal ion/metal systems in the three half cells;Cu= +0.34 VNi= -0.25 VZn= -0.76 VFe(Fe2+)= -0.44 VHence only Zn2+ has a more negative reduction potential than Fe2+. The more negative the reduction potential, the greater the tendency of the system to function as the anode. Thus iron half cell will function as anode in cells 1&2 as explained in the argument above.

Mr. Dayne Senger · Answer

Here are four possible voltaic cells.  Explanation:1. Standard reduction potentials                                          E°/VI₂(s) + 2e⁻ ⟶ 2I⁻(aq);        0.54Cu²⁺(aq) + 2e⁻ ⟶ Cu(s);   0.34Fe²⁺(aq) + 2e⁻ ⟶ Fe(s);   -0.41Zn²⁺(aq) + 2e⁻ ⟶ Zn(s);   -0.762. Possible Voltaic cells(a) Zn/I₂                                                                        E°/V Anode:     Zn(s) ⟶ Zn²⁺(aq) + 2e⁻;                 0.76Cathode:  I₂(s) + 2e⁻ ⟶ 2I⁻(aq);                     0.54 Cell:         Zn(s) +  I₂(s) ⟶  Zn²⁺(aq) + 2I⁻(aq); 1.30Zn(s)|Zn²⁺(aq)∥I⁻(aq)|I₂(s)|C(s, graphite)Zn is the anode; graphite is the cathode.(b) Zn/Cu²⁺                                                                           E°/VAnode:     Zn(s) ⟶ Zn²⁺(aq) + 2e⁻;                    0.76Cathode:  Cu²⁺(aq) + 2e⁻ ⟶ Cu(s);                  0.34Cell:          Zn(s) +  Cu²⁺(s) ⟶  Zn²⁺(aq) + Cu(s); 1.10Zn(s)|Zn²⁺(aq)∥Cu²⁺(aq)|Cu(s)Zn is the anode; Cu is the cathode.(c) Zn/Fe²⁺                                                                             E°/VAnode:     Zn(s) ⟶ Zn²⁺(aq) + 2e⁻;                     0.76 Cathode:  Fe²⁺(aq) + 2e⁻ ⟶ Fe(s);                    -0.41Cell:          Zn(s) +  Fe²⁺(s) ⟶  Zn²⁺(aq) + Fe(s);  0.35Zn(s)|Zn²⁺(aq)∥Fe²⁺(aq)|Fe(s)Zn is the anode; Fe is the cathode.(d) Fe/I₂                                                                          E°/VAnode:     Fe(s) ⟶ Fe²⁺(aq) + 2e⁻;                   0.41Cathode: I₂(s) + 2e⁻ ⟶ 2I⁻(aq);                     0.54 Cell:         Zn(s) +  I₂(s) ⟶  Zn²⁺(aq) + 2I⁻(aq); 0.95Fe(s)|Fe²⁺(aq)∥I⁻(aq)|I₂(s)|C(s, graphite)Fe is the anode; graphite is the cathode.

Anonymous · Answer

i don't knowExplanation:by your mom

Anonymous · Answer

im only 11 but By convention in standard cell notation, the anode is written on the left and the cathode is written on the right. So, in this cell: Zinc is the anode (solid zinc is oxidised). Silver is the cathode (silver ions are reduced).Explanation:

Anonymous · Answer

Overall reaction equationAl(aq) + 3Ag^+(aq)> Al^3+(aq) + 3Ag(s)Explanation:A voltaic cell consists of two half cells; the oxidation half cell( anode) and the reduction half cell(cathode)Anode: Al(aq) > Al^3+(aq) +3eCathode:3Ag^+(aq) +3e > 3Ag(s)Overall reaction equationAl(aq) + 3Ag^+(aq)> Al^3+(aq) + 3Ag(s)The overall reaction equation shows the complete redox reaction taking place in the voltaic cell.

Mr. Richmond Abshire Jr.

All of the following statements concerning voltaic cells are true except 1) oxidation occurs at the cathode. 2) a salt bridge allows

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