The standard potential for given galvanic cell has to be calculated using the standard Gibbs energy value. Concept Introduction: Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation. The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell. The relation between the cell potential E cell and the Gibbs energy is, − ν F E c e l l = Δ r G h e r e , E c e l l − c e l l p o t e n t i a l Δ r G − G i b b s e n e r g y F − F a r a d a y ' s c o nstant ν − n o . o f e l e c t r o n s

Question

Want to see the full answer?

Answer 1

Question

Chapter 5, Problem 5.71P

(a)

Interpretation Introduction

Interpretation:

The standard potential for given galvanic cell has to be calculated using the standard Gibbs energy value.

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is,

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

(b)

Interpretation Introduction

Interpretation:

The standard potential for given couple has to be calculated.

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

A cylinder contains 12 L of water vapour at 150˚C and 5 atm. The temperature of the water vapour is raised to 175˚C, and the volume of the cylinder is reduced to 8.5 L. What is the final pressure of the gas in atmospheres? assume that the gas is ideal

On the next page is an LC separation of the parabens found in baby wash. Parabens are suspected in a link to breast cancer therefore an accurate way to quantitate them is desired. a. In the chromatogram, estimate k' for ethyl paraben. Clearly indicate what values you used for all the terms in your calculation. b. Is this a "good" value for a capacity factor? Explain. c. What is the resolution between n-Propyl paraben and n-Butyl paraben? Again, indicate clearly what values you used in your calculation. MAU | Methyl paraben 40 20 0 -2 Ethyl paraben n-Propyl paraben n-Butyl paraben App ID 22925 6 8 min

d. In Figure 4, each stationary phase shows some negative correlation between plate count and retention factor. In other words, as k' increases, N decreases. Explain this relationship between k' and N. Plate Count (N) 4000 3500 2500 2000 1500 1000 Figure 4. Column efficiency (N) vs retention factor (k') for 22 nonionizable solutes on FMS (red), PGC (black), and COZ (green). 3000 Eluent compositions (acetonitrile/water, A/W) were adjusted to obtain k' less than 15, which was achieved for most solutes as follows: FMS (30/70 A/W), PGC (60/40), COZ (80/20). Slightly different compositions were used for the most highly retained solutes. All columns were 50 mm × 4.6 mm id and packed with 5 um particles, except for COZ, which was packed with 3 um particles. All other chromatographic conditions were constant: column length 5 cm, column j.§. 4.6 mm, flow rate 2 mL/min, column temperature 40 °C, and injection volume 0.5 μL Log(k'x/K'ethylbenzene) FMS 1.5 1.0 0.5 0.0 ཐྭ ཋ ཤྩ བྷྲ ; 500 0 5 10…