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Task 3: In the following problems, you will need to identify the real metals in the electrochemical cells described. You may use each metal more than once or not at all. Choose from the list of six metals: Cu, Ni, Mg, Ag, Fe, or Zn. Standard reduction potentials, E° Ag/Ag* Cu/Cu2+ Ni/Ni²+ Fe/Fe2+ Zn/Zn2+ Mg/Mg2+ + 0.786 V + 0.337 V - 0.249 V - 0.440 V - 0.763 V - 2.370 V Nernst equation at 25°C [Products] [Reactants] 0.059 Ecell = E° log(Q) where Q = cell 3.1 At the anode: 2.0 M visibly blue solution with an orange-brown metal electrode. At the cathode: The 1.0 M solution was colorless and the metal electrode was grey. Cell potential measured: - 1.109 V Clue: both metals form dipositive cations Metal at the anode Metal at the cathode 3.2 At the anode: 0.5 M pale green solution with a grey metal electrode. At the cathode: 2.0 M colorless solution with a grey electrode. Cell potential measured: - 2.103 V Clue: one of the metals is the most active metal in the list (its cation is not easily reduced). Metal at the anode Metal at the cathode 3.3 Observation 1: This metal, when coupled in an electrochemical cell with another grey metal, gives a cell with a standard cell potential of + 1.607 V Observation 2: When this metal is used as an anode, it yields negative AG° values with four out of the six metals. Observation 3: If this metal is coupled with silver in an electrochemical cell, the stochiometric ratio of the metal to Ag is 1:2. Unknown Metal

Task 3: In the following problems, you will need to identify the real metals in the electrochemical cells described. You may use each metal more than once or not at all. Choose from the list of six metals: Cu, Ni, Mg, Ag, Fe, or Zn. Standard reduction potentials, E° Ag/Ag* Cu/Cu2+ Ni/Ni²+ Fe/Fe2+ Zn/Zn2+ Mg/Mg2+ + 0.786 V + 0.337 V - 0.249 V - 0.440 V - 0.763 V - 2.370 V Nernst equation at 25°C [Products] [Reactants] 0.059 Ecell = E° log(Q) where Q = cell 3.1 At the anode: 2.0 M visibly blue solution with an orange-brown metal electrode. At the cathode: The 1.0 M solution was colorless and the metal electrode was grey. Cell potential measured: - 1.109 V Clue: both metals form dipositive cations Metal at the anode Metal at the cathode 3.2 At the anode: 0.5 M pale green solution with a grey metal electrode. At the cathode: 2.0 M colorless solution with a grey electrode. Cell potential measured: - 2.103 V Clue: one of the metals is the most active metal in the list (its cation is not easily reduced). Metal at the anode Metal at the cathode 3.3 Observation 1: This metal, when coupled in an electrochemical cell with another grey metal, gives a cell with a standard cell potential of + 1.607 V Observation 2: When this metal is used as an anode, it yields negative AG° values with four out of the six metals. Observation 3: If this metal is coupled with silver in an electrochemical cell, the stochiometric ratio of the metal to Ag is 1:2. Unknown Metal

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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Task 3: In the following problems, you will need to identify the real metals in the electrochemical cells described. You may use each metal more than once or not at all. Choose from the list of six metals: Cu, Ni, Mg, Ag, Fe, or Zn. Standard reduction potentials, E° Ag/Ag* Cu/Cu2+ Ni/Ni2+ Fe/Fe2+ Zn/Zn2+ Mg/Mg2+ + 0.786 V + 0.337 V - 0.249 V - 0.440 V - 0.763 V - 2.370 V Nernst equation at 25°C [Products] E cell E°c 0.059 log(Q) where Q = cell [Reactants] 3.1 At the anode: 2.0 M visibly blue solution with an orange-brown metal electrode. At the cathode: The 1.0 M solution was colorless and the metal electrode was grey. Cell potential measured: - 1.109 V Clue: both metals form dipositive cations Metal at the anode Metal at the cathode 3.2 At the anode: 0.5 M pale green solution with a grey metal electrode. At the cathode: 2.0 M colorless solution with a grey electrode. Cell potential measured: - 2.103 V Clue: one of the metals is the most active metal in the list (its cation is not easily reduced). Metal at the anode Metal at the cathode 3.3 Observation 1: This metal, when coupled in an electrochemical cell with another metal, gives a cell with a standard cell potential of + 1.607 V Observation 2: When this metal is used as an anode, it yields negative AG° values with four out of the six metals. Observation 3: If this metal is coupled with silver in an electrochemical cell, the stochiometric ratio of the metal to Ag is 1:2. grey Unknown Metal
Transcribed Image Text:Task 3: In the following problems, you will need to identify the real metals in the electrochemical cells described. You may use each metal more than once or not at all. Choose from the list of six metals: Cu, Ni, Mg, Ag, Fe, or Zn. Standard reduction potentials, E° Ag/Ag* Cu/Cu2+ Ni/Ni2+ Fe/Fe2+ Zn/Zn2+ Mg/Mg2+ + 0.786 V + 0.337 V - 0.249 V - 0.440 V - 0.763 V - 2.370 V Nernst equation at 25°C [Products] E cell E°c 0.059 log(Q) where Q = cell [Reactants] 3.1 At the anode: 2.0 M visibly blue solution with an orange-brown metal electrode. At the cathode: The 1.0 M solution was colorless and the metal electrode was grey. Cell potential measured: - 1.109 V Clue: both metals form dipositive cations Metal at the anode Metal at the cathode 3.2 At the anode: 0.5 M pale green solution with a grey metal electrode. At the cathode: 2.0 M colorless solution with a grey electrode. Cell potential measured: - 2.103 V Clue: one of the metals is the most active metal in the list (its cation is not easily reduced). Metal at the anode Metal at the cathode 3.3 Observation 1: This metal, when coupled in an electrochemical cell with another metal, gives a cell with a standard cell potential of + 1.607 V Observation 2: When this metal is used as an anode, it yields negative AG° values with four out of the six metals. Observation 3: If this metal is coupled with silver in an electrochemical cell, the stochiometric ratio of the metal to Ag is 1:2. grey Unknown Metal
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