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- Please write in details on Control of Corrosion and Fuel cell (function and uses).Please do it. Write about control of corrosion and fuel cell and do it please?Given the data below:??2?7 (??)^2− + 14 ?^+ + 6 ?^− → ??(??)^3+ + 7 ?2?(?) ?°??? = 1.33 ???(??)^2+ + 2 ?^− → ??(?) ?°??? = 0.34 ? a. Draw the galvanic cell, including labelling the electrodes and the other portionsof the cell.b. Write the balanced equation for a galvanic cell (balance using the half-reactionmethod, then combine the equations).c. State which half reaction is the cathode and which is the anode.d. Calculate the standard cell potential for this cell.e. Determine the Ecell at 25°C, given: [????? (??)^?−7 ] = ?. ???? ?,[??(??)^?+ ] =?. ???? ?,?? = 5A 40.00 ml aliquot of 0.0500 M HNO2 is diluted to 80.0 ml in water and titrated with 0.0800 M Ce4+ to form NO3- and Ce3+. Assume the hydrogen ion concentration is at 1.00 M throughout the titrtion. Use 1.44 Volts as the standard potential for the Ce4+/Ce3+ system and 0.94 Volts for the NO3-/NO2 system. Write and balance the two half-cell reactions Calculate the potential of the indicator electrode with respect to an Ag/AgCl saturated reference electrode after the titration of the HNO2 solution with 5.00, 50.00, 60.00 and 100.00 ml of Ce4+.
- On the illustration of a generic cell for In/Zn electrodes immersed in their salt solutions Use the Standard Electrode Potential Table. to calculate Eocell (follow this link to find the electrode potential table) https://openstax.org/books/chemistry-atoms-first-2e/pages/l-standard-electrode-half-cell-potentialsBlack-and-white photographic film is coated with silver halides. Because silver is expensive, the manufacturer monitors the Ag⁺ content of the waste stream, [Ag⁺]ᵥᵥₐₛₜₑ, from the plantwith an Ag-selective electrode at 25°C. A stream of known Ag⁺ concentration, [Ag⁺](standard), is passed over the electrode inturn with the waste stream and the data recorded by a computer.(a) Write the equations relating the nonstandard cell potential tothe standard cell potential and [Ag⁺] for each solution.(b) Combine these into a single equation to find [Ag⁺]ᵥᵥₐₛₜₑ.(c) Rewrite the equation from part (b) to find [Ag⁺]ᵥᵥₐₛₜₑ in ng/L.(d) If Eᵥᵥₐₛₜₑ is 0.003 V higher than E(standard), and the standard so-lution contains 1000. ng/L, what is [Ag⁺]ᵥᵥₐₛₜₑ?(e) Rewrite the equation in part (b) to find [Ag⁺]ᵥᵥₐₛₜₑ for a sys-tem in which T changes and Tᵥᵥₐₛₜₑ and T(standard) may be different.I need help writting the net cell equation for this electrochemical cell. I also neeed help calculating ?∘cellEcell∘, Δ?∘rxnΔGrxn∘, Δ?rxnΔGrxn, and ?cellEcell at 25.0 ∘C, thank you.
- A thin circular-disk earring 4.00 cm in diameter is platedwith a coating of gold 0.25 mm thick from an Au³⁺ bath.(a) How many days does it take to deposit the gold on one sideof one earring if the current is 0.013 A (d of gold =19.3 g/cm³)?(b) How many days does it take to deposit the gold on both sidesof the pair of earrings?(c) If the price of gold is $320 per troy ounce (31.10 g), what is the total cost of the gold plating?Please do help me with this please. I promise to give a good feedback.. *Which of the following statements is/are true when standard reduction potential has negative value? i. Oxidation occurs in the half-cell. ii. SHE acted as the oxidation site. iii. At SHE, H2 is oxidized to H+. *In a galvanic cell with a magnesium and gold as half cells, the following describes the characteristic of magnesium. i. Acts as oxidizing agent ii. Reduced in the process iii. Gains electron in the process. *In a galvanic cell with a magnesium and gold as half cells, the following describes the characteristic of gold. i. Acts as oxidizing agent ii. Reduced in the process iii. Gains electron in the process Choice: a. i, iib. ii, iiic. i, iiid. None of the above. Consider a galvanic cell with the anode containing a Zn metal electrode and a 0.10 M Zn(NO3)2solution and the other half-cell containing a Sn metal electrode and a 0.10 M Sn(NO3)2 solution. If themeasured Ecell value is +650 mV and the Zn2+/Zn reduction potential is assumed to be −790 mV, what isthe Sn2+/Sn reduction potential? Show all work.
- The capacity of batteries such as the typical AA alkalinebattery is expressed in units of milliamp-hours (mAh). AnAA alkaline battery yields a nominal capacity of 2850 mAh.(a) What quantity of interest to the consumer is beingexpressed by the units of mAh? (b) The starting voltage of afresh alkaline battery is 1.55 V. The voltage decreases duringdischarge and is 0.80 V when the battery has delivered itsrated capacity. If we assume that the voltage declines linearlyas current is withdrawn, estimate the total maximumelectrical work the battery could perform during discharge.Enter electrons as e-. A voltaic cell is constructed in which the anode is a Sn|Sn2+ half cell and the cathode is a Hg|Hg2+ half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Be sure to 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 migrate _____from/to the Sn|Sn2+ electrode _____fromto the Hg|Hg2+ electrode.In the salt bridge, anions migrate _____fromto the Hg|Hg2+ compartment _____from/to the Sn|Sn2+ compartment.Can you please answer question 1a through 1k? Thanks alot. Nernst Equation: E = E° – (RT/nF) ln Q DGo = -nFEo = -RTlnK 1a. Using Cell Notation and in not more than 2 lines, describe how to make a battery at home from plant source. My Electrolyte = __________________ 1b. Write balanced half-cell and overall equations for the reaction taking place in the described battery in 1. 1c. For the cell above, Calculate the standard electrode potential, Eo, for the balanced redox equation. 1d. Compare the calculated Eo to that of the actual [measured] lemon battery above, what is the % difference? 1e. why are they different? 1f. calculate the Gibbs Free Enegy, DGo,of actual the lemon cell above 1g. Is the cell reaction spontaneous? 1h. Why? 1j. Calculate the Keq for the cell 1k. What is the ratio of the concentration of the [oxidized ion] to that of the [reduced ion] at equilibrium