voltaic cell has been constructed with a nickel metal electrode in Ni- (aq) in one half-cell and a chromium metal electrode etween them and an external wire connecting the metal electrodes completing the circuit. Identify the anode, cathode, and the direction of flow of electrons in the external wire CP (aq) in the other half-cell. The two half-cels ha DA The anode = Cr electrode and the cathode = Ni electrode. The electrons flow from the Ni electrode through the external wire to the Cr electrode. OB. The anode = Ni electrode and the cathode = Cr electrode. The electrons flow from the Cr electrode through the external wire to the Ni electrode. oc The anode = Ni electrode and the cathode = Cr electrode. The electrons flow from the Ni electrode through the external wire to the Cr electrode. On The anode = Cr electrode and the cathode = Ni electrode. The electrons flow from the Cr electrode through the external wire to the Ni electrode.

voltaic cell has been constructed with a nickel metal electrode in Ni- (aq) in one half-cell and a chromium metal electrode etween them and an external wire connecting the metal electrodes completing the circuit. Identify the anode, cathode, and the direction of flow of electrons in the external wire CP (aq) in the other half-cell. The two half-cels ha DA The anode = Cr electrode and the cathode = Ni electrode. The electrons flow from the Ni electrode through the external wire to the Cr electrode. OB. The anode = Ni electrode and the cathode = Cr electrode. The electrons flow from the Cr electrode through the external wire to the Ni electrode. oc The anode = Ni electrode and the cathode = Cr electrode. The electrons flow from the Ni electrode through the external wire to the Cr electrode. On The anode = Cr electrode and the cathode = Ni electrode. The electrons flow from the Cr electrode through the external wire to the Ni electrode.

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

A voltaic cell operating under standard conditions (1.0 M ion concentrations) utilizes the following reaction: What is the effect on the cell emf of each of the following changes? (a) Water is added to the anode compartment, diluting the solution. O The positive cell emf rises, becoming more positive. O The positive cell emf drops closer to zero. O The negative cell emf rises closer to zero. O The negative cell emf drops, becoming more negative. No change in cell emf occurs. (b) The size of the chromium electrode is increased. The positive cell emf rises, becoming more positive. O The positive cell emf drops closer to zero. O The negative cell emf rises closer to zero. O The negative cell emf drops, becoming more negative. O No change in cell emf occurs. x (c) A solution of 1.0 M CrCl3 is added to the anode compartment. The positive cell emf rises, becoming more positive. O The positive cell emf drops closer to zero. O The negative cell emf rises closer to zero. O The negative cell emf…
Consider a galvanic cell with the anode containing a Zn metal electrode and a 0.10M Zn(NO3)2 solution and the other half-cell containing a Sn metal electrode and a 0.10M Sn(NO3)2 solution. If the measured Ecell value is +650mV and the Zn2+/Zn reduction potential is assumed to be -790mV, what is the Sn2+/Sn reduction potential?
Please Help me answer this, thank ue
im a student plz help
A voltaic cell is constructed from a standard Al3+|Al half cell (E°red = -1.660V) and a standard H+|H2 half cell (E°red = 0.000V). The anode reaction is: + + The cathode reaction is: + + The spontaneous cell reaction is: + + The cell voltage is V.
A standard galvanic cell is constructed in which a Pb2+ | Pb half cell acts as the cathode. Which of the following statements are correct? Hint: Refer to a table of standard reduction potentials. (Choose all that apply.) The anode compartment could be I2|I-. The cathode reaction is Pb2+ + 2e- -> Pb Pb is oxidized at the cathode. Pb2+ is reduced at the cathode. In the external circuit, electrons flow from the other compartment to the Pb2+|Pb compartment.
Consider the following cell: | Zn (s) | Ca2* (aq) , SO3²- (aq) || Hg²+ (aq) , F' (aq) | Pt (s) | al Indiate the Oxidizing Agent bindicate the ReducingAge Gont e Wnte he narreattions that occurs ai the cathode d) Write the half reactions that occurs at the anode e) Write the overall net cell reaction f) Calculate the cell potential g) Indicate if electricity is produced or consumed by the cell h) Indicate if the cell is galvanic or electrolytic
The equilibrium constant of the reaction shown below is 2.41x10^8 at 25 degrees Celsius: 3Ag(s) + NO3-(aq) + 4H+(aq) --> 3Ag+(aq) + NO(g) + 2H2O(l) calxulte the value of Ecell for a cell utilizing this reaction
A voltaic cell is constructed from a standard Cu2+|Cu half cell (E°red 0.337V) and %D a standard H+|H2 half cell (E°red 0.000V). %3| The anode reaction is: + + The cathode reaction is: + The spontaneous cell reaction is: + + | The cell voltage is V. + ↑
Use the References to access important values if needed for this question. A standard galvanic cell is constructed in which a Pb2+ | Pb half cell acts as the cathode. Which of the following statements are correct? Hint: Refer to a table of standard reduction potentials. (Choose all that apply.) The anode compartment could be F F. U The anode reaction could be Al -> Al3+ + 3e The cathode reaction is Pb -> Pb2+ + 2e- As the cell runs, anions will migrate from the Pb2"|Pb compartment to the other compartment. O Pb2+ is reduced at the cathode. Submit Answer Try Another Version 3 item attempts remaining
A voltaic cell has been constructed with a nickel metal electrode in Ni2*(aq) in one half-cell and a chromium metal electrode in Cr3+(aq) in the other half-cell. The two half-cells have a saturated KCI bridge between them and an external wire connecting the metal electrodes completing the circuit. Where does oxidation take place and what is the oxidation half-reaction? OA Oxidation takes place in the nickel half-cell: Ni(s) - Ni2*(ag) + 2 e- O B. Oxidation takes place in the nickel half-cell: Ni2*(ag) + 2 e-- Ni(s) O. Oxidation takes place in the chromium half-cell: Cr*(ag) + 3 e- + Cr(s) O D. Oxidation takes place in the chromium half-cell: Cr(s) -+ Cr*(ag) + 3 e-
For the voltaic cell described by the cell reaction below, (1) write the cell diagram, (2) identify which specie is being reduced and which is being oxidized, (3) identify the anode and the cathode, (4) calculate the values of Q, and (5) using the table of standard reduction potentials, show the calculation of the Ecell using the Nernst equation [Ecell = E0cell – (0.0592/n x log Q)]. Zn + Ni+2 (0.10 M) → Zn+2 (0.30 M) + Ni