Consider data from the table of standard reduction potentials for common half-reactions, in your text. For a galvanic cell under standard conditions, which of the following anodic half reactions would produce, at the cathode a spontaneous reduction of Sn4+ to Sn2+ but not Sn2+ to Sn. write yes or no beside each one.     Sn2+ --> Sn4+ + 2e-     H2 + 2OH- --> 2H2O + 2e-     2H- --> H2 + 2e-     H2 --> 2H+ + 2e-     Sn --> Sn2+ + 2e-     Pb + SO42- --> PbSO4 + 2e-

0 A certain half-reaction has a standard reduction potential E 'red must provide at least 0.70 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the anode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? 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. Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used at the cathode of this cell. Note: write the half reaction as it would actually occur at…

Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment): V Pt 0.10 M MnO4 0.40 М Cr3+ 0.20 M Mn2+ 0.30 M Cr,0,2- 0.010 M H* 0.010 MH* The standard reduction potentials are as follows: MnO, + 8H* + 5e → Mn2+ + 4H,O, ɛ° = 1.51 V Cr,0,2- + 14H* + 6e 2Cr** + 7H2O, ɛ° = 1.33 V When current is allowed to flow, which species is oxidized? O Cr,0,²- Cr³+ MnO4 Mn2+ O H*

Consider the cell described below. Al | Al³+ (1.00 M) || Pb²+ (1.00 M) | Pb Calculate the cell potential after the reaction has operated long enough for the [A13+] to have changed by 0.46 mol/L. (Assume T= 25°C.) V Need Help? Read It Supporting Materials Periodic Table Watch It Constants & Factors Supplemental Data

Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the concentration of the ion at the anode is 0.500 M and the concentration of the ion at the cathode is 1.50 M. Use the standard reduction potentials from Appendix L in our textbook.

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A standard galvanic cell is constructed with Cu2+ | Cu+ and Cl2 | Cl- half cell compartments connected by a salt bridge. Which of the following statements are correct? Hint: Refer to a table of standard reduction potentials. (Choose all that apply.) -In the external circuit, electrons flow from the Cl2|Cl- compartment to the Cu2+|Cu+ compartment. -The anode compartment is the Cl2|Cl- compartment. -As the cell runs, anions will migrate from the Cl2|Cl- compartment to the Cu2+|Cu+ compartment. -Cu+ is oxidized at the anode. -The cathode compartment is the Cl2|Cl- compartment.

Do not have to answer any questions. JUST WRITE THE OBJECTIVES IN YOUR OWN RODS: Objective: To measure Ecel for several voltaic cells and determine the standard potential for each half cell. To determine Ksp of AgCl and the K of [Cu(NH3)4]*.

Please answer all parts - thank you!

Use smallest possible integer coefficients. If a box is not needed, leave it blank. Use a table of Standard Reduction Potentials to predict if a reaction will occur between Hg metal and I,(s), when the two are brought in contact via standard half-cells in a voltaic cell. If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank.