The oxidation of methanol, as described by the equation below, has a ΔGo value of -937.9 kJ/mol. What is the standard cell potential for a methanol fuel cell? 2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(l) a) 0.810 V b) 9.72 V c) -9.72 V d) 0.405 V e) -2.43 V

The potential in an electrochemical cell, E, is related to the Gibb's free energy change (ΔG) for the overall cell redox reaction:(1) ΔG0 = -nFE0where n is the number of electrons transferred during the redox reaction, F is Faraday's constant (96,500 C / mol), and the superscript 0 indicates standard conditions (1 atm, 1 M concentrations, and 25 °C). Thus, a measurement of the cell voltage at standard conditions can be used to determine ΔG0.As an example, the following cell reaction:Zn(s)+Cu2+(aq) →Zn2+(aq)+Cu(m)generates a cell voltage of +1.10V under standard conditions. Based on the example from the previous section, calculate and enter below ΔG0 (with 3 sig figs) for this reaction in kJ/mol.

A galvanic (voltaic) cell consists of an electrode composed of iron in a 1.0 M1.0 M iron(II) ion solution and another electrode composed of copper in a 1.0 M1.0 M copper(I) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C.25 °C. Refer to the list of standard reduction potentials.

Consider a fuel cell that uses the reaction of ethanol with oxygen to produce electricity. CH, CH,OH(1) + 30,(g) → 2 CO,(g) + 3 H,O(1) Use thermodynamic data to determine the value of Ea for this cell at 25 °C. Eall = V 'cell

Consider a galvanic cell that uses the reaction Zn(s) + 2H+(aq) →Zn2+(aq) + H2(g) Calculate the cell potential at 25oC when [H+] = 1,0 M, [Zn2+] = 0.0010 M and pH2 = 0.10 atm

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 1.00 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? Data O yes, there is a minimum. E red = v 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. O no minimum Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? O yes, there is naximum. Pred = Iv 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. no maximum By using the information…

Consider the voltaic Cell shown below. Voltaic Cell V Voltmeter Salt Ag (s)-> bridge Cd (s) Ag+ (aq) 2.75 M Cd+2 (aq) 0.0125 M • What is the value of potential for the spontaneous reaction that occurs as the cell operates at 25°C? Ecell = • As the cell operates spontaneously under these conditions, which electrode is the cathode of the cell? Cd Ag • Which Electrode loses mass as the cell operates under these conditions? Ag Cd

A certain half-reaction has a standard reduction potential E=+0.43 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that red must provide at least 1.50 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 cathode of the cell. O-0 Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? Ov O yes, there is a minimum. red 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. O no minimum 27 Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? Ov O yes, there is a maximum. 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. O no maximum

When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic cell in which solid lead(II) sulfate (PBSO4) is reduced to lead at the cathode and oxidized to solid lead(II) oxide (PbO) at the anode. Suppose a current of 46.0 A is fed into a car battery for 24.0 seconds. Calculate the mass of lead deposited on the cathode of the battery. Round your answer to 3 significant digits. Also, be sure your answer contains a unit symbol.

Consider the voltaic cell with a standard cell potential of 0.150 V. What is the cell potential of the voltaic cell at 400 K? Cd(s) | Cd2+ (1.00 x 10-4 M) || Ni2+ (0.100 M) | Ni(s) R= 8.314 J/mol-K; F = 96,485 J/mol-V