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1.) The standard potential from tables for two half reactions are given below. Sn (aq) + 2 e → Sn(s) -0.136 V Ni (aq) + 2 e » Ni(s) -0.257 V Calculate the expected cell potential using SHE standard values provided for the following combinations, a. Sn/Sn and Ni/Ni*2 V b. Calculate the following cell potentials using half-cell potential of Zn given in the lab write up and given here as: Zn+2 + 2 e → Zn E° = -0.763 V Sn/Sn*2 and Zn/Zn*2 V Ni/Ni2 and Zn/Zn*2 175

1.) The standard potential from tables for two half reactions are given below. Sn (aq) + 2 e → Sn(s) -0.136 V Ni (aq) + 2 e » Ni(s) -0.257 V Calculate the expected cell potential using SHE standard values provided for the following combinations, a. Sn/Sn and Ni/Ni*2 V b. Calculate the following cell potentials using half-cell potential of Zn given in the lab write up and given here as: Zn+2 + 2 e → Zn E° = -0.763 V Sn/Sn*2 and Zn/Zn*2 V Ni/Ni2 and Zn/Zn*2 175

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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1.) The standard potential from tables for two half reactions are given below. Sn (aq) + 2 e Sn(s) -0.136 V Ni (aq) + 2 e » Ni(s) -0.257 V Calculate the expected cell potential using SHE standard values provided for the following combinations. a. Sn/Sn and Ni/Ni*2 b. Calculate the following cell potentials using half-cell potential of Zn given in the lab write up and given here as: Znt2 + 2 e → Zn E° = -0.763 V Sn/Sn*2 and Zn/Zn*2 V Ni/Ni*2 and Zn/Zn*2 V 175
Transcribed Image Text:1.) The standard potential from tables for two half reactions are given below. Sn (aq) + 2 e Sn(s) -0.136 V Ni (aq) + 2 e » Ni(s) -0.257 V Calculate the expected cell potential using SHE standard values provided for the following combinations. a. Sn/Sn and Ni/Ni*2 b. Calculate the following cell potentials using half-cell potential of Zn given in the lab write up and given here as: Znt2 + 2 e → Zn E° = -0.763 V Sn/Sn*2 and Zn/Zn*2 V Ni/Ni*2 and Zn/Zn*2 V 175
e. Using the cell potentials in b.), calculate the potentials for each half reaction if you used a Zn "Standard" rather than the SHE Remember that you must identify the cathode correctly as either the Zn or the other metal. To do this, decide on the cathode and anode such that you obtain a "" voltage for the cell. Sn/Sn2 Ni/Ni*2 E° = d. Using your new standard, calculate the cell voltage if these two substances were used to produce a voltaic cell. Compare with the SHE results in part a. e. Identify, from the cell constructed each of the following. Circle One for each. Sn Cell Ni Cell Cathode Sn Ni Substance being Oxidized Sn Cell Ni Cell Cell to which K* flow from the salt bridge. f. Write the overall cell reaction: g. What would have happened if we had used the Fe/Fe*2 half reaction as a standard instead of Zn? What would have and have not changed? 176
Transcribed Image Text:e. Using the cell potentials in b.), calculate the potentials for each half reaction if you used a Zn "Standard" rather than the SHE Remember that you must identify the cathode correctly as either the Zn or the other metal. To do this, decide on the cathode and anode such that you obtain a "" voltage for the cell. Sn/Sn2 Ni/Ni*2 E° = d. Using your new standard, calculate the cell voltage if these two substances were used to produce a voltaic cell. Compare with the SHE results in part a. e. Identify, from the cell constructed each of the following. Circle One for each. Sn Cell Ni Cell Cathode Sn Ni Substance being Oxidized Sn Cell Ni Cell Cell to which K* flow from the salt bridge. f. Write the overall cell reaction: g. What would have happened if we had used the Fe/Fe*2 half reaction as a standard instead of Zn? What would have and have not changed? 176
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