[References) A solution containing Pt** is electrolyzed with a current of 3.20 A. How long will it take to plate out 99% of the platinum in 0.10 L of a 0.010-M solution of Pt+? Time Submit Answer Try Another Version 1 item attempt remaining

[References) A solution containing Pt** is electrolyzed with a current of 3.20 A. How long will it take to plate out 99% of the platinum in 0.10 L of a 0.010-M solution of Pt+? Time Submit Answer Try Another Version 1 item attempt remaining

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter22: An Introduction To Electroanalytical Chemistry

Section: Chapter Questions

Problem 22.18QAP

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Calculate the minimum difference in standard electrode potentials needed to lower the concentration of the metal M1 to 2.00 10-4 M ¡n a solution that is 1.00 10-1 M in the less-reducible metal M2 where (a) M2 is univalent and M1 is divalent. (b) M2 and M1 are both divalent, (c) M2 is trivalent and M1 is univalent, (d) M2is divalent and M1 is univalent, (e) M2 is divalent and M1 ¡s trivalent.
Quinone undergoes a reversible reduction at a voltammetric working electrode. The reaction is (a) Assume that the diffusion coefficients for quinone and hydroquinone are approximately the same and calculate the approximate half-wave Potential (versus SCE) for the reduction of hydroquinone at an RDE from a solution buffered to a pH of 8.0. (b) Repeat the calculation in (a) for a solution buffered to a pH of 5.0.
Táke off any gridlines and add a title and axes labels. Add the trendline and the relevant equation. b) If a sample was analyzed and the current was measured to be 5.18 mA, what is the concentration of analyte in the sample? 5.18= 3.403x + 1.9232 3.2368=3.4403 x 0.947: x Pentane (C5H12) is a liquid with density of 0.929 g/mL at 25 °C. Find the true mass of pentane when the mass in air is 14.82 g. Assume air density is 0.0012 g/mL.
Pls help ASAP. Pls show all work and caluclations.
Solve 2 please
Calculate the cell potential of a cell operating with the following reaction at 25°C in which [Cr2O72] = 0.040 M , I] = 0.025 M, [Cr**] = 0.10 M, and [H*] = 0.45 M. %3D Cr2 O,2 (ag) + 6I (aq) + 14H+ (aq) → 2Cr³+ (aq) + 3I2 (s) + 7H2O(1) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard Half-Reaction Potential, E° (V) I2 (s) + 2e = 21 (aq) 0.54 Cr2 O,2 (aq) + 14H† (aq) + 6e¯ = 2Cr** (aq) + 7H2O(1) 1.33 Cell potential = V
Solve 1 and 2 please
Please help me answer #2. Answer written on bracket. Thank you.
Please Help!! Part A: Electrochemical Cell Mass Data for Electochemical Cell Copper Zinc Initial mass of strip (g) 2.421 2.436 Final mass of strip (g) 2.602 2.250 Measured Ecell (V)= 1.02 Part B: Electroplating Mass Data for Electoplating Mass (g) Initial 0.930 After first plating 1.083 After second plating 1.238 After third plating 1.377 Part A: Electrochemical Cell Table view List view Mass Calculations for Electochemical Cell Copper Zinc Initial mass of strip (g) 2.421 2.436 Final mass of strip (g) 2.602 2.250 Mass gained(+) or lost(−) (g) 0.18 -0.19 what is Computed Ecell (V)? what is Computed ΔG (kJ/mol)? Mass Calculations for Electroplating (fill in chart) First Second Third Final mass of paper clip (g) 1.083 1.238 1.377 Initial mass of paper clip (g) 0.930 1.083 1.238…
i Assignment Score: 18.5% AA Question 3 of 13 > Macmillan Learning E = 0.7 assessments.macmillanlearning.com Incorrect Resources Feedback Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+] = 0.840 M and [Fe2+] = 0.0150 M. Use the standard reduction potentials in this table. Cr(s) + Fe²+ (aq) = Cr²+ (aq) + Fe(s) Try Again Attempt 2 V
14.) What mass of Mn(s) may be deposited from an aqueous MnCl2 solution if a current of 2.50 A is applied to the solution for 365 s? (ε°red(Mn2+/Mn) = -1.185 V, F = 96485 C/mol) a. 0.219 g b. 0.520 g c. 0.308 g d. 1.04 g e. 0.260 g
Please show all work and calculations. thank you