1. How long it takes to deposit 20.4 grams of gold (197 g/mol) when 5.6 ampere current was passed(aq) + 3e → Au(s)through its Au*3 aqueous solution? Au*3F = 9.65 x 104 Coulombs/moles ofes2. Use the following information, calculate the molar mass of metal “X" and use the periodic table toidentify the metal: When 1.24 amps current passed thru it's XCI aqueous solution for 1.5 hours,5.93 grams of metal X was deposited. {keep in mind the CI-1 has -1 charge and molar mass of XCI =mass/number of moles so first calculate the mass then molar mass}

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1. How long it takes to deposit 20.4 grams of gold (197 g/mol) when 5.6 ampere current was passed through its Au*3 aqueous solution? Au* (aq) + 3e → Au(s) F = 9.65 x 104 Coulombs/moles of es

1. How long it takes to deposit 20.4 grams of gold (197 g/mol) when 5.6 ampere current was passed through its Au3 aqueous solution? Au (aq) + 3e → Au(s) F = 9.65 x 104 Coulombs/moles of es

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

1. How long it takes to deposit 20.4 grams of gold (197 g/mol) when 5.6 ampere current was passed
(aq) + 3e → Au(s)
through its Au*3 aqueous solution? Au*3
F = 9.65 x 104 Coulombs/moles of
es
2. Use the following information, calculate the molar mass of metal “X" and use the periodic table to
identify the metal: When 1.24 amps current passed thru it's XCI aqueous solution for 1.5 hours,
5.93 grams of metal X was deposited. {keep in mind the CI-1 has -1 charge and molar mass of XCI =
mass/number of moles so first calculate the mass then molar mass}

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