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1.) The standard potential from tables for two half reactions are gven below Sn (aq) + - Sn(s) 0.136 V Ni (aq) - Ni(s) 20 6.257 V a. Calculate the expected cell potential using SHE standard values provided for the following combinations. Sn/Sn and Ni/NI 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/Sn2 and Zn/Zn2 Ni/Ni*2 and Zn/Zn*2

1.) The standard potential from tables for two half reactions are gven below Sn (aq) + - Sn(s) 0.136 V Ni (aq) - Ni(s) 20 6.257 V a. Calculate the expected cell potential using SHE standard values provided for the following combinations. Sn/Sn and Ni/NI 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/Sn2 and Zn/Zn2 Ni/Ni*2 and Zn/Zn*2

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
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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e. Using the cell potentials in b.), calculate the potentials for each half reaction if VOu 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 "+" votage for the cell. Sn/Sn Ni/Ni V. E° = V 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. Cathode Sn Cell Ni Cell Substance being Oxidized Sn Ni Cell to which K* flow from the salt bridge. Sn Cell Ni Cell 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 VOu 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 "+" votage for the cell. Sn/Sn Ni/Ni V. E° = V 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. Cathode Sn Cell Ni Cell Substance being Oxidized Sn Ni Cell to which K* flow from the salt bridge. Sn Cell Ni Cell 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
1.) The standard potential from tables for two half rections are given below. Sn (aq) + 5 Sn(s) 0.136 V Ni (aq) + 2e Ni(s) 0.257 V Calculate the expected cell potential using SHE standard vaes provided for the following combinations. a. Sn/Sn and Ni/Ni 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/Snt2 and Zn/Zn*2 Ni/Ni*² and Zn/Zn*2 V 175
Transcribed Image Text:1.) The standard potential from tables for two half rections are given below. Sn (aq) + 5 Sn(s) 0.136 V Ni (aq) + 2e Ni(s) 0.257 V Calculate the expected cell potential using SHE standard vaes provided for the following combinations. a. Sn/Sn and Ni/Ni 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/Snt2 and Zn/Zn*2 Ni/Ni*² and Zn/Zn*2 V 175
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