sing two doubly-clipped wires, he LED with the cathode of the end of the same LED with the nd see if the LED lights up. If discuss how you can change LED light up. You may need groups. The goal is to make Try the other LED after you The first one. porous cup and return it to solid waste. Use tongs to solid waste container. Do as the ions are hazardous. Calculations Practice Problem 1: Which reaction will occur spontaneously? a) a manganese strip in tin(II) solution or b) a tin strip in manganese(II) solution? Answer: a ■Practice Problem 2: A galvanic cell is constructed using two half-cells: Bi(s) in 0.1 M Bi(NO3)3(aq) and Zn(s) in 0.1 M ZnSO4(aq). The two half cells are connected by a KNO3 salt bridge and two copper wires from the electrodes to a voltmeter. Which one will be the anode: Bi(s) or Zn(s)? What is the standard cell potential? Write the cell diagram (line notation) for this cell. Answer: Zn has the lower Ered so it will be the anode where oxidation takes place. Ecell = Eox + Ered= -(-0.7618 V)+(0.308 V) = 1.069 V. Zn(s) | ZnSO4(aq, 0.1 M) || Bi(NO), (aq, 0.1 M) | Bi(s)

sing two doubly-clipped wires, he LED with the cathode of the end of the same LED with the nd see if the LED lights up. If discuss how you can change LED light up. You may need groups. The goal is to make Try the other LED after you The first one. porous cup and return it to solid waste. Use tongs to solid waste container. Do as the ions are hazardous. Calculations Practice Problem 1: Which reaction will occur spontaneously? a) a manganese strip in tin(II) solution or b) a tin strip in manganese(II) solution? Answer: a ■Practice Problem 2: A galvanic cell is constructed using two half-cells: Bi(s) in 0.1 M Bi(NO3)3(aq) and Zn(s) in 0.1 M ZnSO4(aq). The two half cells are connected by a KNO3 salt bridge and two copper wires from the electrodes to a voltmeter. Which one will be the anode: Bi(s) or Zn(s)? What is the standard cell potential? Write the cell diagram (line notation) for this cell. Answer: Zn has the lower Ered so it will be the anode where oxidation takes place. Ecell = Eox + Ered= -(-0.7618 V)+(0.308 V) = 1.069 V. Zn(s) | ZnSO4(aq, 0.1 M) || Bi(NO), (aq, 0.1 M) | Bi(s)

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...

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