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Use Equation 5 and the Standard Reduction Potentials table to determine which statement is true. Remember that any spontaneously operating cell has a positive E° cell value. Copper is the anode and lead is the cathode. O Zinc is the cathode and lead is the anode. O Aluminum is the cathode and zinc is the anode. OZinc is the cathode and copper is the anode. Aluminum is the cathode and lead is the anode. Copper is the anode and aluminum is the cathode. O Aluminum is the cathode and copper is the anode. O Copper is the cathode and zinc is the anode.

Use Equation 5 and the Standard Reduction Potentials table to determine which statement is true. Remember that any spontaneously operating cell has a positive E° cell value. Copper is the anode and lead is the cathode. O Zinc is the cathode and lead is the anode. O Aluminum is the cathode and zinc is the anode. OZinc is the cathode and copper is the anode. Aluminum is the cathode and lead is the anode. Copper is the anode and aluminum is the cathode. O Aluminum is the cathode and copper is the anode. O Copper is the cathode and zinc is the anode.

Chemistry
Chemistry
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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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Use Equation 5 and the Standard Reduction Potentials table to determine which statement is true. Remember that any spontaneously operating cell has a positive E° cell value. OCopper is the anode and lead is the cathode. Zinc is the cathode and lead is the anode. O Aluminum is the cathode and zinc is the anode. O Zinc is the cathode and copper is the anode. Aluminum is the cathode and lead is the anode. O Copper is the anode and aluminum is the cathode. O Aluminum is the cathode and copper is the anode. O Copper is the cathode and zinc is the anode.
Transcribed Image Text:Use Equation 5 and the Standard Reduction Potentials table to determine which statement is true. Remember that any spontaneously operating cell has a positive E° cell value. OCopper is the anode and lead is the cathode. Zinc is the cathode and lead is the anode. O Aluminum is the cathode and zinc is the anode. O Zinc is the cathode and copper is the anode. Aluminum is the cathode and lead is the anode. O Copper is the anode and aluminum is the cathode. O Aluminum is the cathode and copper is the anode. O Copper is the cathode and zinc is the anode.
Table of Reduction Potentials REACTION E° (V) Li* (aq) + e > Li (s) -3.04 Al3+ (aq) + 3e > Al (s) -1.66 2 H20 (1) + 2e > H2 (g) + 2 OH (aq) -0.83 Zn2+ (aq) + 2e → Zn (s) -0.76 Cr3* (aq) + 3e → Cr (s) -0.74 Fe2* (aq) + 2e Fe (s) -0.45 Ni2* (aq) + 2e Ni (s) -0.26 Pb2+ (aq) + 2e → Pb (s) -0.13 Fe3+ (aq) + 3e → Fe (s) -0.04 2H* (aq) + 2e > H2 (g) 0.00 Cu2* (aq) + 2e → Cu (s) +0.34 O2 (g) + 4 H* (aq) + 4e >2 H20 (I) +1.23 E"cel = E'red (cathode) - E"red (anode) (5) Where the superscript zero refers to standard conditions (1 M concentrations) We will use Eq. 5 along with the reduction potentials in Table 1 to calculate the expected standard cell potentials for this experiment. As noted above, the expected cell voltage (potential) for nonstandard conditions (Ecen) depends on the concentrations of the aqueous solutions involved. The relationship for this (known as the Nerst Equation) is
Transcribed Image Text:Table of Reduction Potentials REACTION E° (V) Li* (aq) + e > Li (s) -3.04 Al3+ (aq) + 3e > Al (s) -1.66 2 H20 (1) + 2e > H2 (g) + 2 OH (aq) -0.83 Zn2+ (aq) + 2e → Zn (s) -0.76 Cr3* (aq) + 3e → Cr (s) -0.74 Fe2* (aq) + 2e Fe (s) -0.45 Ni2* (aq) + 2e Ni (s) -0.26 Pb2+ (aq) + 2e → Pb (s) -0.13 Fe3+ (aq) + 3e → Fe (s) -0.04 2H* (aq) + 2e > H2 (g) 0.00 Cu2* (aq) + 2e → Cu (s) +0.34 O2 (g) + 4 H* (aq) + 4e >2 H20 (I) +1.23 E"cel = E'red (cathode) - E"red (anode) (5) Where the superscript zero refers to standard conditions (1 M concentrations) We will use Eq. 5 along with the reduction potentials in Table 1 to calculate the expected standard cell potentials for this experiment. As noted above, the expected cell voltage (potential) for nonstandard conditions (Ecen) depends on the concentrations of the aqueous solutions involved. The relationship for this (known as the Nerst Equation) is
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