If the free energy of an electrochemical process is +12 kJ/mol and n=3, what is the standard cell potential for the process?

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…

The Nickel-Cadmium battery cell has a standard potential of 1.2 V. What is the standard free energy change for this reaction?

what is the standard cell potential (in Volts) for a a galvanic cell that can do 567 kJ of work. The number of electrons tranferred in the rxn is 4.

Write the balanced chemical equation for the spontaneous redox reaction. Include states of matter. Calculate the standard cell potential.  If the initial concentrations of Zn2+ and of OH– are 1.0 × 10–7 and 2.0 × 10–7, respectively, calculate the cell potential after the Zn2+ concentration has increased by a factor of 100. At this point, what percentage of the initial voltage remains?

I need to find standard cell potential, the non-standard cell potential, using [Au^+]= 0.0015M and [Fe^3+]= 0.033M.  I need to calculate Gibb's free energy and equilibrium constant, K.  Is the reaction spontaneous or nonspontaneous?  Are reactants or products favored at equilibrium under non-standard conditions?

The free energy change for the following reaction at 25 °C, when [H*] = 3.34x103 M and [Hg+] = 1.15 M, is 180. kJ: 2H*(3.34x103 M) + Hg(1)→ H2(g) + Hg²*(1.15 M) AG = 180. kJ What is the cell potential for the reaction as written under these conditions? Answer: Would this reaction be spontaneous in the forward or the reverse direction?

The triprotic form of the amino acid cysteine is shown below, along with the pK, value for each ionizable site. The isoelectric point (pl) for cysteine occurs at pH= 5.1. B 10.8 CH₂ SH C13 A LA -OH (1) What is the charge on the molecule at the isoelectric point? (2) In the predominant form of the molecule at the isoelectric point, is each of the sites (labeled A, B, and C) protonated or unprotonated? site A site B: site C

A quantity of electricity equal to 6.95 × 104 C passes through an electrolytic cell that contains a solution of Sn4+(aq) ions. Compute the maximum chemical amount, in moles, of Sn(s) that can be deposited at the cathode.

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ Cu2+ (aq) + Zn (s) → Cu (s) + Zn²+ (aq) 2+ Suppose the cell is prepared with 3.51 M Cu²*+ in one half-cell and 1.20 M Zn²+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 日 ☐ x10 ☐ μ ロ・ロ