Table 1.
Cathode Cu, Anode Al, Ecell °= 0.337 - (-1.662) = 1.992V
2Al(s) + 3Cu2+(aq) ------> 3Cu(s) + 2Al3+(aq)
Cathode Zn, Anode Al, Ecell° = -0.7618 -(-1.662) = 0.9002V
2Al(s) + 3Zn2+(aq) -----> 3Zn(s) + 2Al3+(aq)
Sn anode, Cu cathode, Ecell°= 0.337- (-0.13) = 0.467V
Sn(s) + Cu2+(aq) ------> Sn2+(aq) + Cu(s)
Slope of the graph is -2.303RT/ nF
= - 2.303× 8.314×298/2×96485 = - 0.029
Post-Laboratory Report (Page 1/1) Group Number Date: Day Time 1. The salt bridge in Goal #1 was s...
rading Time Dav Experiment#7: Electrochemical Cells Part II. Cu" Concentration Cell [Cu2+] of the stock solution: 02 ' Potential difference for various concentration cells. (- ) 0.5 M 0.05 M 0.005 M 0.0005 M 0.5 M 045 . O 88 0.05 M .0252 0.005 M 0.0005 M Concentration Difference Concentration Ratio Log(Conc. Ratio)Measured Potential 0.5 M/0.05 M 0.5 M/0.005 M 0.5 M/0.0005 M Attach 3 graphs: (1.) Ecell vs. Concentration Difference; (2) Ecell vs. Concentration Ratio; (3) Ecell vs. log(Conc....
E° (cal.) E° (exp.) 1. Fe(s)| Fe2+ (1 M) || Cu2+ (1 M) | Cu(s) 0.775 V 2. Pb(s) Pb2+ (1 M) || Cu2+ (1 M) Cu(s) 0.461 V 3. Sn(s) | Sn2+ (1 M) || Cu2+ (1 M) | Cu(s) 0.472 V 4. Zn(s) | Zn2+ (1 M) || Cu2+ (1 M) Cu(s) 1.095 V 5. Zn(s) | Zn2+ (1 M) || Cu2+ (1 M + NH3) | Cu(s) 0.928 V a) The Nernst equation for the cell in...
Candidate l: Zn(s) | Zn2+(aq,0.500 M) I Cu2+(aq, 1.00 M) Cu(s) Candidate 2: Pb(s) | Pb2+(aq, 0.500 M) || Cu2+(aq, 1.00 M) Cu(s) Candidate 3: Mg(s) | Mg2+(aq, 0.500 M) | Pb2+(aq, 1.00 M)| Pb(s) (a) 6 pts) Choose one of the candidate voltaic cells #1, #2, or #3. Draw a schematic cell diagram for the candidate voltaic cell of choice. Clearly label anode, cathode, electrodes, ions and their concentrations, salt bridge, and the flow of electrons. (b) (5 pts)...
need help with 10& 11 LUPIJFyldtebook%252Fdo%252Fstudent%252FviewGrades%3Fcourse_id%3D_7145... O Selected Answer: 2 Q 100% - Reset Question 9 0.5 out of 0.5 points The cell potential for the electrochemical cell in question #6 is measured at 0.426 V. Using the potential calculated for the copper half reaction in question 114, calculate the reduction potential for the Fe3+. Fe2+ half-reaction. Selected Answer: 766 Question 10 O out of 1 points Use the Nernst equation to calculate the expected cell potential (cell) for the...
Page 1 and 2 are instructions. Please help me solve K for page 3 and page 4 and please check the other work on Page 3. Thanyou very much. Will Rate! CHM 112 Electrochemical Cells and Thermodynamics Section A. Constructing a Small-Scale Electrochemical Cell Woodbridge Campus Objective To construct a small-scale electrochemical cell using a redox system, to measure the cell potential and derive thermodynamic quantities. Procedures 1. Connect the red and black alligator clips to the multimeter to read...
The following problems are based upon the following voltaic cell (concentration of aqueous solutions are 1 M): (Show all work for full credit.) Fe (s) Fe" (aq) | |Cu (aq) | Cu (s) (3) 1. The reduction potential for the iron half reaction is -0.040 v. Use your textbook to determine the reduction potential for the copper half reaction, and record that here. )2. From the voltaic cell written above, which half cell will be the anode, and which will...
C-1. DETERMINE THE E° FOR A VOLTAIC CELL For each cell write the anode half reaction and the cathode half reaction. From the measured voltages, calculate the half-cell potentials for the lead and tin half-cells and the equilibrium constants for these two reactions. In these calculations, use E° = 0.34 V for the Cu2+/Cu couple. Cell trial 1 trial 2 trial 3 Cu-Pb 0.505 V 0.506 V 0.508 V Cu-Sn 0.688 V 0.688 V 0.691 V Pb-Sn 0.190 V 0.190...
A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(I), [Cu(NH). If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.074 V at 298 K Constants Periodic Table Use the standard reduction potentials shown here to answer the questions Reduction half-reaction E (V) Cu2+ (aq) 2e Cu(s) 0.337 2H + (aq) + 2e →H, (g) | 0.000 ▼ Part A...
need help with the rest of the table EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE To determine the standard cell potential values of several electrochemical coll INTRODUCTION The basis for an electrochemical cell is an oxidation reduction Corredor be divided into two half reactions reaction. This reaction can Oxidation half reaction Gloss of electrons) takes place at the anode, which is the positive electrode that the anions migrate to Chence the name anode) Reduction half reaction (gain of electrons)...
Question 1. Use the data you collected from the video to calculate how many voltaic cells are there in Battery #5: This is a lithium battery battery? Question 2. Use the data you collected from the video to calculate how many voltaic cells are there in Battery #6: This is an alkaline battery battery? Data- I also have two questions below.. I already answered them I just want to double check that my answers are correct! Thank you! Measured Voltaic...