Determine work (AG) that the non-standard voltaic cell below can produced. Pt| Cl2 (s) | Cl- (1.00 M) || F- (2.25 M) | F2(s) | Pt. • give answer in kJ units. 3 significant figures with the negative sign. Example: -3.568 kJ should be written as a final answer of -3.57. The standard half reduction reactions and corresponding potentials are: F2(s) + 2 e- → 2 F-(aq) E' = +2.866 V Cl2(s) + 2 e- → 2 Cl-(aq) E° = 1.358 V work = AG = - z F Ecel. F= 96485 J/mol e V

Enter electrons as e". A voltaic cell is constructed in which the anode is a Ag Ag" half cell and the cathode is a Hg Hg* half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coeficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is: In the external circuit, electrons migratel the AgAg" electrode v the Hg Hg* electrode. In the salt bridge, anions migrate| v the Hg|Hg" compartment| v the AgAg" compartment. +

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…

Give the balanced cell equation and determine & for the galvanic cells based on the following half-reactions. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) H₂O2 + 2H+ + 2e → 2H₂O € = 1.78 V Cr₂O7²- + 14H+ + 6e¯ →2 Cr³+ + 7H₂O €° = 1.33 V a. b. € = V € = + 2H+ + 2e → H₂ → Al A1³+ +3e V € = 0.00 V € = -1.66 V