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In part A of Expt. 10, we were going to construct some simple galvanic cells. The...
In Part B we were going to construct concentration cells. In these galvanic cells, the driving force is the difference in concentration in the two half-cells. Write the anode and cathode reactions for a concentration cell which contains 0.1 M Cu2+ in one half-cell and 0.01 M Cu2+ in the other. (Be clear as to which [Cu2+] is being oxidized or reduced).
7. You decide to construct a zinc/aluminum galvanic cell in which the electrodes are connected by a wire and the solutions are connected with a salt bridge. One electrode consists of an aluminum bar in a 1.0 M solution of aluminum nitrate. The other electrode consists of zinc bar in a 1.0 M solution of zinc nitrate. Draw the complete electrochemical cell diagram and use it to answer the questions that follow. a. Which electrode is the cathode and which...
B1. Construction of Galvanic Cells a. For each galvanic cells you construct, calculate the theoretical cell potential using the table of the Standard Electrode Potentials from the Chemistry 0130 data booklet. (3 marks) Measured Galvanic Cells Cathode reaction Anode reaction Voltage (V) Cu?*/Cu and Zn/Zn? 0.937 v Zn/Zn2+ and Ag /Ag 1.329v Ag"/Ag and Cu/Cu2+ 0.394v Electrochemistry 9 b. For each galvanic cells, write the overall cell reaction (balanced net ionic equation). • identify the oxidizing agent (OA) and reducing...
data collected Cu(NO3)2 | Zn(NO3)2 = 0.999 V Pb | 1.0 M Pb(NO3)2 || 1.0 M Zn(NO3)2 | Zn = 0.396 V PART B: REDUCTION POTENTIALS 1. Report the measured cell potential for each galvanic cell and state which electrode corresponds to the cathode and which to the anode. 2. Given E = -0.76 V for the Zn/Zn half-cell, and your measured Ecell, calculate the reduction potential at the Cu and Pb electrodes and write the redox half- 6 reactions...
3. Two galvanic cells were constructed, as shown below. 1.61 0.88 KINO a. Which lead (red or black) is attached to the cathode and which is attached to the anode? How do you know? (5 pts) b. Write the line notation and cell reaction for the Ag/X cell. (5 pts) c. Given that the X(s) electrode is in a 0.10 M XCl2 solution, calculate the standard reduction potential for (5 pts) X2(aq) + 2e → X)
Part A through H 1. [60 pts) A galvanic cell is a type of battery where the electrodes are immersed in different electrolyte solutions, which are connected by an ion-conducting bridge. Consider a galvanic cell with Al and Cu electrodes. The Al electrode is immersed in a solution containing a standard concentration of Al3+ ions and the Cu electrode is immersed in a solution containing a standard concentration of Cu* ions. External Circuit The standard reduction potentials for the half...
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which is the anode, and calculate the cell potential. (Use the table of Standard Electrode Potentials.) (a) Ca(II) and Sc(III) Cathode: . Ca(II) Sc(III) Anode: Ca(II) Sc(III) Ecell = 0.0591 x V (b) Pb(II) and In(III) Cathode: . Pb(II) In(III) Anode: Pb(II) In(III) Ecell - (c) Ni(II) and Zr(IV) Cathode: NI(II) Zr(IV) Anode: Ni(II) Zr(IV) Ecell - V Supporting Materials Periodic Table Supplemental...
In a galvanic cell, one half-cell consists of a lead strip dipped into a 1.00 M solution of Pb(NO3)2. In the second half-cell, solid uranium is in contact with a 1.00 M solution of U(NO3)3. Pb is observed to plate out as the galvanic cell operates, and the initial cell voltage is measured to be 1.672 V at 25°C. (a) Write balanced equations for the half-reactions at the anode and the cathode. Show electrons as e-. Use the smallest integer...
some questions are filled out but still need help woth the remainder of this assignment part B and below needs to be answered. Paragraph Styles . . Electrochemical Cells Objective: Investigate electrochemical potential using electrochemical cells. Information: Electric current is the flow of negatively charged particles. An electrochemical cell is a device that creates an electric current by converting chemical energy into electric current, or vice versa. Voltaic cells are electrochemical cells that produce current spontaneously by converting chemical energy...
Mcasured Cell Potentials of Redo x Couples from cells A1. A2, Bl. B2, and Unknown #1 Redox Measured Anode Anode Reaction Cathode Cathode Reaction CouplePotential Cu-Zn 10.qqv|Zn |2n→ (Al-B2) Cu-Pb Pb-Zn (BI-B2) 0-46V Fe-Pb Fe-Zn Cu-Fe (AI-A2) Zn-Unk#1 (B2-A3) 0.3Iv Unkel Assuming that the reduction potential for Zn2 (0.10 M/Zn is equal to -0.79 V, calculate the reduction potentials for the remaining cells: Cu (0.10 M/Cu 0.2ov Calculation: 95 0- 0.71-0.20V zn ls) 2 ทั้า(o.1o)11 Fe2+Co.10m) 1 Fecz) Fe (0.10...