Cyclic Voltammogram of 10mM Ruthenium Hexamine 40 20 -20 -40 -60 -0.4 -0.2 0.0 0.2 potential (V) The half-wave potential for the reverse scan of the cyclic voltammogram is approximately . O- 0.17 V O -0.21 V -0.075 V -0.25 V -0.5 V current (uA)

Cyclic Voltammogram of 10mM Ruthenium Hexamine 40 20 -20 -40 -60 -0.4 -0.2 0.0 0.2 potential (V) The half-wave potential for the reverse scan of the cyclic voltammogram is approximately . O- 0.17 V O -0.21 V -0.075 V -0.25 V -0.5 V current (uA)

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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||| ELECTROCHEMISTRY Calculating standard reaction free energy from standard... Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 4 significant digits. 5Cu* (aq) + MnO4 (aq) + 8H* (aq) → 5Cu²+ (aq) + Mn²+ (aq) + 4H₂O0 (1) 0x X S A Netflix ? G CH3(ch2... D Hannah V 8 Olh 8:
Consider the electrolysis reactions cathode Cu²+ (aq, 0.125 M) + 2e anode H₂O(1) = whose standard reduction potentials can be found in this table. Calculate the voltage needed to drive the net reaction if the current is negligible. Ecell = Cu(s) 10₂(g, 1 bar) + 2 H+ (aq, 0.243 M) + 2€¯ The cell has a resistance of 63.0 and a current of 7.26 mA when the cathode overpotential is 0.223 V and the anode overpotential is 0.084 V. Calculate the voltage needed to overcome these effects and drive the net reaction. Ecell = V V
both questions go together... thanks! Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) F2(g) + 2 e- 2 F-(aq) 2.87 Ce4+(aq) + e- Ce3+(aq) 1.61 MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O(l) 1.51 Cl2(g) + 2 e- 2 Cl-(aq) 1.36 Cr2O72-(aq) + 14 H+(aq) + 6 e- 2 Cr3+(aq) + 7 H2O(l) 1.33 O2(g) + 4 H+(aq) + 4 e- 2 H2O(l) 1.229 Br2(l) + 2 e- 2 Br-(aq) 1.08 NO3-(aq) + 4 H+(aq) + 3 e- NO(g) + 2 H2O(l) 0.96 2 Hg2+(aq) + 2 e- Hg22+(aq) 0.920 Hg2+(aq) + 2 e- Hg(l) 0.855 Ag+(aq) + e- Ag(s) 0.799 Hg22+(aq) + 2 e- 2 Hg(l) 0.789 Fe3+(aq) + e- Fe2+(aq) 0.771 I2(s) + 2 e- 2 I-(aq) 0.535 Fe(CN)63-(aq) + e- Fe(CN)64-(aq) 0.48 Cu2+(aq) + 2 e- Cu(s) 0.337 Cu2+(aq) + e- Cu+(aq) 0.153 S(s) + 2 H+(aq) + 2 e- H2S(aq) 0.14 2 H+(aq) + 2 e- H2(g) 0.0000 Pb2+(aq) + 2 e- Pb(s) -0.126 Sn2+(aq) + 2 e- Sn(s) -0.14 Ni2+(aq) + 2 e- Ni(s) -0.25…
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Given the standard electrode reduction potentials, which reaction will occur spontaneously?
Write out the complete equation for the chemical reaction that occurred when you joined the cups together to make a voltaic cell. Make sure the equation is balanced.
Calculate the expected Ecell for each galvanic cells. Reduction potential of Zn2+(0.1 M)/Zn half-cell: –0.79 V Procedure Pipet 1 mL of the 0.1 M Cu(NO3)2 solution (Solution 1) from the Zn2+(0.1 M)/Zn half-cell into a 50 mL volumetric flask and dilute to the mark with deionized water. Pour this diluted solution (Solution 2) into a 50 mL beaker. Pipet 1 mL of Solution 2 into a 50 mL volumetric flask and dilute to the mark with deionized water. Pour this diluted solution (Solution 3) into a 50 mL beaker. Repeat using Solution 3 to prepare Solution 4. Measure the cell potential for each of the three galvanic cells that can be made by pairing the Zn2+(0.1 M)/Zn half-cell with the half-cells containing Solutions 2–4 and the copper electrode.
Please complete the table and provide the calculations and steps to determine the standard E^o values in the table.
please answer a b c