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- Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the following solutions to 1.00 10-6 M (assume reaction product in each case is elemental Hg): (a) an aqueous solution of Hg2+? (b) a solution with an equilibrium SCN- concentration of 0.100 M? Hg2+ + 2SCN- Hg(SCN)2(aq) = Kf = 1.8 107 c) a solution with an equilibrium Br- concentration of 0.100 M? HgBr42++ 2e- Hg(l) + 4Br- E0= 0.223 VCalculate the emf at 298.15 K generated by the oxidation of Fe2+ by O2 in acidic solution, according to the following reaction: O2(g) + 4H+(aq) + 4Fe2+(aq) ⟶ 4Fe3+(aq) + 2H2O(l) when [H+] = 0.003 M, [Fe3+] = 2.5 x 10 – 4 M, and [Fe2+] = 0.18 M. Also, write the complete (oxidation/reduction) half-reactions.
- The measured cell potential, ?cellEcell, for the cell shown is −0.3605−0.3605 V at 25 ∘C25 ∘C. Calculate the H+H+ concentration. Pt(s) | H2(g,0.825 bar) | H+(aq,? M) || Cd2+(aq,1.00 M) | Cd(s)Pt(s) | H2(g,0.825 bar) | H+(aq,? M) || Cd2+(aq,1.00 M) | Cd(s) The balanced reduction half-reactions for the cell and their respective standard reduction potential values, ?∘E∘, are given. 2H+(aq)+2e−⟶H2(g)?∘Cd2+(aq)+2e−⟶Cd(s)?∘=0.00 V=−0.403 VMany applications of electrochemistry have been in chemical analysis.Suppose a Fe|Fe2+ concentration cell is set-up in which the [Fe2+] = 1.0 x10¯2 M in one compartment but the concentration in the othercompartment is unknown. The Ecell was measured at 0.024V when thehalf-cells were connected.(i) Without doing a numerical calculation, is the unknown more orless concentrated than the 1.0 x 10¯2 M solution? Justify youranswer(ii) Calculate the unknown concentration.(iii) Does your calculated answer agree with your original answer?Why?Many applications of electrochemistry have been in chemical analysis.Suppose a Fe|Fe2+ concentration cell is set-up in which the [Fe2+] = 1.0 x10¯2 M in one compartment but the concentration in the othercompartment is unknown. The Ecell was measured at 0.024V when thehalf-cells were connected.(i) Without doing a numerical calculation, is the unknown more orless concentrated than the 1.0 x 10¯2 M solution? Justify youranswer
- The standard reduction potential (Eo) for the conversion of Cr2O72- to Cr3+ at 25 degree C in an aqueous solution of pH 3.0 is 1.33 V. The concentrations of Cr2O72- and Cr3+ are1.0 × 10-4 M and 1.0 × 10-3 M, respectively. Then the potential of this half-cell reaction is (Given: Faraday constant = 96500 C mol1, Gas constant R = 8.314 J K1 mol1)The E°cell = 0.135 V for the reaction3I2(s) + 5Cr2O72-(aq) + 34H+(aq) → 6IO3-(aq) + 10Cr3+(aq) + 17H2OWhat is Ecell if [Cr2O72-] = 0.014 M, [H+] = 0.21 M, [IO3-] = 0.00018 M, and [Cr3+] = 0.0039 M?Ecell =If a dilute H2 SO4 solution is electrolyzed with copper electrodes, the most likely electrode reactions are 2H ^ + + 2e- = H2 (g) at the cathode and 2Cu (s) + H2O = Cu2O (s) + 2H ^ + + 2e- at the anode. If we observe the formation of 27.4 cm3 of moist hydrogen (751 barometric torrs, 23.3 ° C) at the cathode, what change in weight will there be simultaneously at the anode? Data: Pv H2O 23.3 ° C = 22 torr.Atomic mass: Cu (65); O (16); H (1)
- Black-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 want all questions answered Consider the cell: Pt|H₂(g,p°)| HCl(aq)|AgCl(s)|Ag for which the cell reaction is 2AgCl(s) +H₂(g) → 2 Ag(s) + 2HCl(aq). At 25 °C and a molality of HCl of 0.010 mol kg⁻¹ . Calculate ionic strength of solution?Calculate (in volts) Standard Electrode Potential of the cell E°:?Calculate (in kJ/mol) Standard Gibbs Free Energy of the cell ΔrG°?Assuming Debye-Huckel limiting law holds at this concentration, calculate (in volts) Ecell (Cl⁻, AgCl, Ag)? Assuming Debye-Huckel limiting law holds at this concentration, calculate (in kJ) ΔrG?. Answer the following questions:a. Write the two electrochemical half reactions for a solid oxide fuel cell showing how CO can be utilized as a fuel in the SOFC.b. A solid-oxide fuel cell runs on methane (CH4) and produces heat and electricity.Assuming that the current output of the fuel cell is j = 1 A∕cm2 and voltage V = 0.6 V, calculate the required fuel cell active area (in cm2) to produce 3 kW of electrical power? c. The change in enthalpy and Gibbs free energy Δh and Δg for methane combustion at the standard operating condition of the fuel cell (750 oC, 1 atm), are (–802) and (–801)kJ/mol, respectively. Assuming 100% fuel utilization, what is the rate of heat generation by the fuel cell (Pheat, in kW) when operated at j = 1 A∕cm2 and V = 0.6 V?
