ssignment Score: AA tion 3 of 13 > Macmillan Learning E = 0.7 18.5% Incorrect assessments.macmillanlearning.com Resources Feedback Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+] = 0.840 M and [Fe²+] = 0.0150 M. Use the standard reduction potentials in this table. Cr(s) + Fe²+ (aq) = Cr²+ (aq) + Fe(s) Try Again Attempt 2 V

ssignment Score: AA tion 3 of 13 > Macmillan Learning E = 0.7 18.5% Incorrect assessments.macmillanlearning.com Resources Feedback Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+] = 0.840 M and [Fe²+] = 0.0150 M. Use the standard reduction potentials in this table. Cr(s) + Fe²+ (aq) = Cr²+ (aq) + Fe(s) Try Again Attempt 2 V

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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A certain half-reaction has a standard reduction potential E=+0.21 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.30 V of electrical power. The cell will operate under standard conditions. l Data Note for advanced students: assume the engineer requires this half-reaction to happen at t Half-Reaction E° (V) Ag+ (aq) + e + Ag (s) A13+ (aq) + 3e - Al (s) Au+ (aq) + e - Au (s) Au3+ (aq) + 3e - Au (s) 0.7996 -1.676 Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? O yes, there is a minimum. E = Ov 1.692 1.498 If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Ba2+ (aq) + 2e- - Ba (s) -2.912 O no minimum Br2 (1) + 2e - 2Br (aq) 1.066 Ca2+ (aq) + 2e-- Ca (s) -2.868 Cl2 (g) + 2e - 2CI (aq) Co2+ (aq) + 2e-- Co (s) Co3+ (aq) + e - Co2+ (aq) Cr2+ (aq) + 2e → Cr (s) Cr3+ (aq) + 3e +…
Calculate the cell potential (Ecell) for the following lead concentration cell at 298 K.
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Given the standard electrode reduction potentials, which reaction will occur spontaneously?
True or False: The reaction, S₂082- + Ni(OH)2 + 2OH2SO42- + NiO2 + 2H₂O, will occur spontaneously under standard state conditions. Following are the standard reduction potentials that may be useful: NiO2 + 2H₂O +2e=Ni(OH)2 +2OH E = 0.49 V S2082 +2e=2SO4²- True False E° = 2.01 V
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You are given an electrochemical cell where the chemical reaction involves a silver complex. A silver metal bar is used as the positive electrode. The electrochemical potential for this cell is given by E=EºAg+/Ag-0.0592(volts)*log(1/[Ag+]) For a test solution with a silver concentration of 0.001 M, the electrochemical cell potential is 0.20 volts. Find the silver electrode potential EºAg+/Ag. This same cell from (a) is used to measure the electrochemical potential for a new silver complex in equilibrium. If the measured cell potential is 0.324 volts, what is the silver concentration for this new silver complex at equilibrium?
Table 1 Selected standard reduction potentials for half-reactions red measured in Reduction Half-Equation E° red, V Mg2+(aq) + 2e→ Mg(s) -2.37 Al3+(aq) + 3 e → Al(s) -1.66 Cr²+(aq) + 2e → Cr(s) -0.91 Zn2+(aq) + 2e → Zn(s) -0.76 Fe2+(aq) + 2e → Fe(s) -0.44 Ni²+(aq) + 2e → Ni(s) -0.26 Sn2+(aq) + 2e → Sn(s) -0.14 Pb2+(aq) + 2 e → Pb(s) -0.13 2 H+(aq) + 2e → H2(g) 0.00 Cu2+(aq) + 2e→ Cu(s) +0.34 Ag+(aq) + e Ag(s) +0.80
please answer a b c