Objective: Determine the flow of electrons in a battery (voltaic cell) Identify the anode and cathode in a voltaic cell Voltaic Cells (batteries) Directions: In each of the following, determine which element oxidized easier on table J (higher up on table J). Then label the anode, cathode, direction of e- flow, (remember electrons flow from high to low), which electrode increases and decreases in mass and then write the half reactions in the spaces provided. Voltmeter Voltaic Cell Switch Wire Wire- Voltmeter Wire Salt Salt bridge -Ag(s) electrode Cu(s) electrode- Al(s) electrode bridge Ni(s) electrode Cu2 (aq) Ag+(aq) AI(NO),(aq) Ni(NO),(aq) Cu(s) + 2Ag-(aq) Cu2 (aq) + 2Ag(s) 2A[(s) + 3Nf*(aq) → 2A*(aq) + 3Ni(s) 1. 2. oX: oX: red: red: Voltaic Cell V Wire Switch Voltmeter Voltmeter Wire Salt Mg(s) electrode Cu(s) electrode Salt bridge bridge Ag(s) Ni(s) Mg2 (aq) Cu2+(aq) Ag*(aq) Ni?"(aq) Mg(s) + Cu2+(aq) → Mg2+(aq) + Cu(s) 3. 4. OX: ox: red: red:

Objective: Determine the flow of electrons in a battery (voltaic cell) Identify the anode and cathode in a voltaic cell Voltaic Cells (batteries) Directions: In each of the following, determine which element oxidized easier on table J (higher up on table J). Then label the anode, cathode, direction of e- flow, (remember electrons flow from high to low), which electrode increases and decreases in mass and then write the half reactions in the spaces provided. Voltmeter Voltaic Cell Switch Wire Wire- Voltmeter Wire Salt Salt bridge -Ag(s) electrode Cu(s) electrode- Al(s) electrode bridge Ni(s) electrode Cu2 (aq) Ag+(aq) AI(NO),(aq) Ni(NO),(aq) Cu(s) + 2Ag-(aq) Cu2 (aq) + 2Ag(s) 2A[(s) + 3Nf(aq) → 2A(aq) + 3Ni(s) 1. 2. oX: oX: red: red: Voltaic Cell V Wire Switch Voltmeter Voltmeter Wire Salt Mg(s) electrode Cu(s) electrode Salt bridge bridge Ag(s) Ni(s) Mg2 (aq) Cu2+(aq) Ag*(aq) Ni?"(aq) Mg(s) + Cu2+(aq) → Mg2+(aq) + Cu(s) 3. 4. OX: ox: red: red:

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

Fill in the Blank
Which of the following statements are true about the cathode during the operation of a voltaic electrochemical cell? © Metal cations can deposit as the corresponding metal on the surface of the cathode The cathode is positively charged with respect to the anode. The cathode is where the reduction reaction occurs. In a salt bridge, the positively charged ions flow towards the cathode. Onlv two of the above four statements are true Only three of the first four statements above are true. All of the first four statements above are true.
Use the given galvanic cell notation below to answer the following questions. 2+ Sn (s) | Sn²+ (aq) || Ti+ (aq)| Ti (s) a) Write the oxidation half reaction. Balance and include states. b) Write the reduction half reaction. Balance and include states. c) Write the overall cell reaction. Balance and include states. d) Identify the anode and cathode. Label your answers a), b), c), d).
What are the names/ IUPAC
please answer #5 type the answer or write it clearly so i can understand please
Please answer within 10 minutes
A galvanic (voltaic) cell is made using the 2 half cells: Zn2+ (aq) + 2e → Zn(s) E =-.763 V Mg2+ (aq) + 2e - → Mg(s) with Zn(s) and Mg(s) as the electrodes. Answer the questions A. It is the anode. [Select ] B. It is the cathode. [Select] C. Electrons in the wire flow toward it. [Select]. D. Anions from the salt bridge flow toward it. [Select] E. Gains mass. [Select] E = -2.37 V F. Losses mass. [Select]
14
Consider a galvanic cell created from the following redox reaction: 3Zn (s) + 2Au3+ (aq) → 3Zn2+ (aq) + 2Au (s) 1) Draw out a schematic diagram (as shown in image) 2) Label each component (anode, cathode, salt bridge, solution choice, and electron flow direction) in your schematic diagram.
A voltaic cell consists of an aluminum electrode in a solution of Al(NO3)3 in one beaker, and, in the other beaker, of a platinum electrode immersed in a KCl solution, with Cl2 gas bubbled around it. A salt bridge connects the two aqueous solutions and a metallic wire connects the two electrodes. a) Write the oxidation half-reaction b) Write the reduction half-reaction. c) Write the overall balanced equation d) Which electrode serves as the anode? e) Does the aluminum electrode lose or gain mass as the cell reaction proceed? f) Calculate the standard cell potential Ecell at 25 oC.
Please send me the question in 20 minutes it's very urgent plz
Need both of these