Example: A steel coupon with an anode surface area of 1000 cm2 is placed in an electrolyte. The corrosion current is measured to be 1 mA. What mass of steel will be lost in 6 hours? What is the corrosion rate in ug /cm2/day? In mpy? Assume valence of 2, atomic weight = 55 847 g and o = 720 x 106ug (cm3

Example: A steel coupon with an anode surface area of 1000 cm2 is placed in an electrolyte. The corrosion current is measured to be 1 mA. What mass of steel will be lost in 6 hours? What is the corrosion rate in ug /cm2/day? In mpy? Assume valence of 2, atomic weight = 55 847 g and o = 720 x 106ug (cm3

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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6) Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If a current of 6.0A and a voltage of 4.5V are used: Cr20, (aq) + 14H* (aq) + 12e- → 2Cr() + 7H20 a) How many hours would it take to completely convert 215mL of 1.25M K2C12O7 to elemental chromium? b) How many kilowatt-hours of electrical energy are required to plate 1.00 g of chromium?
The balanced half-reaction occuring at the cathode in the redox reaction shown below is 3MNO 4(aq) +24Hag) + 5Fe(s) → 3Mna + 5Fe + 12H20) 7(aq) Caqg) + 5Fe?+ (aq) + 12H200 O Fe(s) + Fe + 3e (aq) O MnOa(ag) +8H + 5e → Mn? + 4H20O (aq) (aq) O Feo +3e -→ Fe(s) eaq) O Mn + 4H20u→ MnOalag) + 8Hi) + 5e (aq) + 4H2OW→ MnOA(aqg) + 8H + 5e- (aq)
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A current of 0.600 A is passed through an electrolytic cell containing molten KBr for 2.50 h. How much product will be formed at the anode? 2Br + 2K+ → Br₂ + 2K MM of K = 39.10 g/mol MM of Br₂ = 159.8 g/mol R = 8.314 J/mol-K F = 96,485 J/mol-V O 1.09 g O 4.47 g O 8.94 g O 2.19 g
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A solution of Cdl2 having a molality of 0.007545 mol/kg was electrolyzed in a Hittorf cell. The mass of cadmium deposited at the cathode was 0.03462 g. A solution weighing 152.64 g was withdrawn from the anode compartment and was found to contain 0.3818 g of Cdl2. Calculate the transport numbers of Cd²+ and 1¹.
White gold is regular gold electroplated with rhodium. An object is electroplated with rhodium for 28.2 minutes at at current of 1.4 A. Rh3+ + 3 e Rh Molar mass Rh = 102.9 g/mol %3D F = 96,485.34 C/mol e A = C/s Given the information above, calculate how many grams of rhodium should theoretically be plated on the object. IMPORTANT: When entering your answer: • Enter the number only (no units) • Do not leave any spaces • Use a leading zero before the decimal when necessary Report your number to 3 decimal places (regardless of the significant figures) Correctly round your answer to the 3rd decimal place (margin of allowed error is only + 0.001, so always use un-rounded numbers in your calculations) Examples: 0.123 or 9.876
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Copper was electroplated from a Cu2SO4 solution onto an electrode with an active surface area of 5.97 cm2. Determine the thickness (mm) of the deposit if the current is kept constant at 3.41 A for 0.7415 hours. (density of Cu = 8.96 g/cm3, MW of Cu = 63.55 g/mol)
Copper was electroplated from a Cu2SO4 solution onto an electrode with an active surface area of 3.83 cm2. Determine the thickness (mm) of the deposit if the current is kept constant at 3.94 A for 1.4466 hours. (density of Cu = 8.96 g/cm3, MW of Cu = 63.55g/mol). Input values only with 2 decimal places. Do not include the unit.
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