Chapter 31, Problem 2ASA

ELECTROCHEMISTRY: Copper was electroplated from a CuzSO4 solution onto an electrode with an active surface area of 4.27 cm. Determine the thickness (mm) of the deposit if the current is kept constant at 3.5 A for 0.8432 hours. (density of Cu = 8.96 g/cm, MW of Cu = 63.55 g/mol). (input values only with 2 decimal places. Do not include the unit.)

Molten RbCl can be electrolyzed to form metallic Rb. For what duration should an electrolysis be performed at a current of 2.53 A in order to produce 18.7 g Rb? _______________s

ELECTROCHEMISTRY: Copper was electroplated from a Cu2S04 solution onto an electrode with an active surface area of 7.17 cm-. Determine the thickness (mm) of the deposit if the current is kept constant at 3.42 A for 1.4748 hours. (density of Cu = 8.96 g/cmo, MW of Cu = 63.55 g/mol). (Input values only with 2 decimal places. Do not include the unit.)

ELECTROCHEMISTRY: Copper was electroplated from a Cu2SO4 solution onto an electrode with an active surface rea of 3.19 cm2. Determine the thickness (mm) of the deposit if the current is kept constant at 4.53 A for 0.8715 hours. (density of Cu = 8.96 g/cm3, MW of Cu = 63.55 g/mol). (Input values only with 2 decimal places. Do not include the unit.)

ELECTROCHEMISTRY: Copper was electroplated from a Cu2SO4 solution onto an electrode with an active surface area of 7.17 cm2. Determine the thickness (mm) of the deposit if the current is kept constant at 3.42 A for 1.4748 hours. (density of Cu = 8.96 g/cm3, MW of Cu = 63.55 g/mol). (Input values only with 2 decimal places. Do not include the unit.)   show sol'n please

QUESTION 8 ELECTROCHEMISTRY: Copper was electroplated from a Cu2SO4 solution onto an electrode with an active surface area of 7.55 cm. Determine the thickness (mm) of the 3 deposit if the current is kept constant at 4.61 A for 0.9284 hours. (density of Cu = 8.96 g/cm, MW of Cu = 63.55 g/mol). (Input values only with 2 decimal places. Do not include the unit.)

Consider a ring which was electroplated with gold (Au, MM = 197 g/mol) using an Au(III) salt with a 0.328-Ampere current for 4.00 min. R= 8.314 J/mol-K; F = 96,485 J/mol-V 1. How much electric charge passed through the cell? [Select] V II. How many moles of electrons passed through the cell? [Select] III. How much gold were deposited onto the ring? [Select] V V

Copy down the potential from the diagram above, as shown on the voltmeter: ___1.10_______ V Note: Voltage (V) is a measurement of the electrochemical potential or “electromotive force” (e.m.f.), how charged particles are being pushed in one direction or another. In the case of the copper/zinc electrochemical battery, the 1.10 V means that each Coulomb (C) of electric charge will gain an energy of 1.10 Joule (J) (1 V = 1 J/C). For reference, 1 electron has a charge of 1.602 x 10-19 C (or 1 mole of electrons carry about 100,000 C of electric carge).The common data of electrochemical potential is in the form of standard reduction potential tables, like the one shown below (similar to Table 17.1 in OpenStax):   ****Note that the reduction of H+ to become H2 is set as 0.00 V. The electrode made of this combination is called the standard hydrogen electrode (SHE), and standard reduction data is usually presented with respect to SHE. One intuitive way to understand the standard reduction table…

QUESTION 4 ELECTROCHEMISTRY: Copper was electroplated from a Cu2SO4 solution onto an electrode with an active surface area of 7.43 cm. Determine the thickness (mm) of the deposit if the current is kept constant at 3.8 A for 0.9142 hours. (density of Cu = 8.96 g/cm3, MW of Cu = 63.55 g/mol). (Input values only with 2 decimal places. Do not include the unit.) QUESTION 5