The nickel-cadmium, or NiCad battery, is one of the first rechargeable batteries. Cadmium metal forms one electrode while a powder of nickel oxide hydroxide (NIO(OH)) is pressed onto an inert carbon electrode to form the other. Using standard cell notation, the cell is represented by Cd(s) | Cd(OH)2(s) | OH(aq) | NIO(OH)(s) | Ni(OH)2(s) | C(s) Which one of the following statemers is FALSE regarding the operation of the battery? Cadmium hydroxide is being formed at the anode. Ni(OH)2 is produced at the cathode. The nickel ions are being reduced to the +3 oxidation state. Electrons flow from the anode to the cathode. Cadmium metal is being consumed.

The nickel-cadmium, or NiCad battery, is one of the first rechargeable batteries. Cadmium metal forms one electrode while a powder of nickel oxide hydroxide (NIO(OH)) is pressed onto an inert carbon electrode to form the other. Using standard cell notation, the cell is represented by Cd(s) | Cd(OH)2(s) | OH(aq) | NIO(OH)(s) | Ni(OH)2(s) | C(s) Which one of the following statemers is FALSE regarding the operation of the battery? Cadmium hydroxide is being formed at the anode. Ni(OH)2 is produced at the cathode. The nickel ions are being reduced to the +3 oxidation state. Electrons flow from the anode to the cathode. Cadmium metal is being consumed.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)
Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized to Mg2+ (aq) and a cathode where Ag+ (aq) is reduced to Ag (s) . Assume all aqueous solutions have a concentration of 1 mol/L.
What is the net reaction for the cell? Is it .44V or .22V?
A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Br2(1) + Mn(s) 2Br"(aq) + Mn2+(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: Enter the reaction that takes place at the cathode. Include state symbols: In the external circuit, electrons migrate the Mn electrode the Br2 electrode. Anions migrate the salt bridge the Br2 compartment.
A cell at 25oC is described by the following cell notationZn(s) | Zn2+(aq) || Zn2+(aq) | Zn(s)The concentration of zinc ions at the cathode is 0.50M while the concentration of zinc ions at the anode is 0.10M. Based on the given cell notation and concentrations, (show proper units and box final answers)A) Calculate the standard free energy change.B) Calculate the cell potential.C) If the given concentrations of zinc ions for anode and cathode are reversed, will the reaction proceed forward or backward?
Which statement is correct for the cell with a notation Pt /Cl2(g)/Cl¯(aq) // Zn+2(aq)/Zn ? choose 1 Neither of the anode and cathode is a standard hydrogen electrode. The cathode is a standard hydrogen electrode. The anode is a standard hydrogen electrode.
Write the cell notation for an electrochemical cell consisting of an anode where Ni (s) is oxidized to Ni2+ (aq) and a cathode where Cu2+ (aq) is reduced to Cu (s) . Assume all aqueous solutions have a concentration of 1 mol/L.
Write the cell notation for an electrochemical cell consisting of an anode where Sn (s) is oxidized to Sn2* (aq) and a cathode where Cu²* (aq) is reduced to Cu (s). Assume all aqueous solutions have a concentration of 1 mol L.
Write the cell notation for an electrochemical cell consisting of an anode where Cu (s) is oxidized to Cu²+ (aq) and a cathode where Fe³+ (aq) is reduced to Fe²+ (aq) at a platinum electrode. Assume all aqueous solutions have a concentration of 1 mol/L.
Silver metal can be dissolved in acidic solutions via a redox reaction with generation of hydrogen gas. Which of the following is the correct cell notation for the reaction that will occur?
Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized to Mg2+ (aq) and a cathode where Cr3+ (aq) is reduced to Cr2+ (aq) at a platinum electrode . Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.
Consider this cell diagram for an electrochemical cell: Pt(s) | H2(g) | H*(aq) || Cu*(aq) | Cu(s) What is the overall balanced reaction for this redox reaction? O 2H (aq) + 2Cu(s) H2(g) + 2Cu (aq). O H2(g) + 2Cu'(aq) → 2H*(aq) + 2Cu(s) O H2(g) + 2Cu(s)H'(aq) + 2Cu'(aq) O H2(g) + Cu (aq) H'(aq) + Cu(s)