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- In a polarographic experiment of a 60 mL of 0.08 M Cu2+solution, a limitingcurrent was left on for 15 minutes. If the average current during the time of theexperiment is 6.0 μA, what fraction of the copper is removed from the solution? TheFaraday constant is 96485 C/mol of electron.Calculate the measured current density for metal M when immersed in boiling water, it's found that the anodic potential is 0.2 V and cathodic potential is 0.09 V, and the exchange current density is 20 mA / m'.q = 0.5Pb 2+ +2e−→PbE ∘ =1.69 V If PbF 2 is dissolved in water, a Pb∣Pb 2+ ∥SCE reads 1.37 V. What is the Ksp of PbF 2 ?
- The mobility of a Li+ ion in an aqueous solution is 4.01×10−8 m2s−1 V−1 at 25°C. The potential difference between two electrodes in the solution placed 1.0 cm apart is 12.0 V. What is the lithium ion current rate? (Use μms-1 for your answer)1) Calculate the mass of metal that is plated when an electrolytic cell consisting of aqueous tantalum(III) chloride and a tantalum electrode runs for 16.00 h with at current of 200.5 A. 2)A chemical reaction at standard thermodynamic temperature with a rate constant of 6.13×10−2 M−1 s−1 and an initial reactant concentration of 0.446 M, is heated to 414.3 ∘C. If the activation energy of the reaction is 32.76 kJ mol−1, how many times faster is the reaction at the higher temperature with the same initial concentration?In a voltammogram, which of the following statements is correct 2 a. The limiting current i, is used for quantitative analysis b. The half-wave potential E₁/2 is used for quantitative analysis c. The limiting current i depends on the identity of the analyte d. The half-wave potential E1/2 dependens on the analyte concentration A 0.20 g sample of primary standard Na₂C₂O4 (134 g/mol) needed 37.22 mL of of KMnO4 solution to reach the end point. What is the molarity of KMnO4 reagent a. 0.14 M b. 0.016 M C. 0.65 M d. 0.0014 M In the glucose sensor, the component diffuses through the inner layer of the electrode is the J a. gluconic acid b. hydrogen peroxide c. glucose d. glucose oxidase
- Given a cell: 2 Ag+(aq) + Cu(s) ----> 2Ag (s) + Cu2+ (aq), E(cell) = 0.346 V, E0(cell) = E0cathode - E0anode = 0.800 V - 0.340 V = 0.460 V, I. calculate the concentration of Cu2+ given that of Ag+ is 1.0 x 10-5M Cu2+M= Keq =Given a cell: 2 Ag+(aq) + Cu(s) ----> 2Ag (s) + Cu2+ (aq), E(cell) = 0.346 V, E0(cell) = E0cathode - E0anode = 0.800 V - 0.340 V = 0.460 V, I. calculate the concentration of Cu2+ given that of Ag+ is 1.0 x 10-5MCalculate the potential of an alloy (Ni) electrode immersed in Ni(OH)2, pH = 9.00, Ksp = 6.5 × 10-18
- The following cell was employed for the determination of pCrO4: SCE // CrO4 2-(xM) / Ag2CrO4 (s) / Ag (s) Find the pCrO4 if the cell potential is - 0.402 V (E0 Ag/Ag2CrO4 = - 0.316 V ; E SCE = 0.241 V)The following cell was used for the determination of pCrO4: SCE||CrO42- (xM), Ag2CrO4 (sat’d)|Ag Calculate pCrO4 if the cell potential is 0.386.Propagation of uncertainty. In an extremely accurate measurement of the Faraday constant, a pure silver anode was oxidized to Ag1 with a constant current of 0.203 639 0 (60.000 000 4) A for 18 000.075 (60.010) s to give a mass loss of 4.097 900 (60.000 003) g from the anode. Given that the atomic mass of Ag is 107.868 2 (60.000 2), find the value of the Faraday constant and its uncertainty.
