9. Chromium plating is applied by electrolysis to objects suspended in a dichromate solution, according to this half-reaction: Cr20,2 (aq) + H*(aq) + e¯ -> Cr(s) + H2O(I) (unbalanced) How long (in hours) would it take to apply a chromium plating 0.010 mm thick to a car bumper with a surface area of 0.32 m² in an electrolytic cell carrying a current of 25.0 A and assuming electrolysis is 88% efficient? The density of chromium is 7.19 g/cm³. AW of Cr = 52. A. 0.54 h B. 1.25 h C. 2.42 h D. 3.23 h

9. Chromium plating is applied by electrolysis to objects suspended in a dichromate solution, according to this half-reaction: Cr20,2 (aq) + H*(aq) + e¯ -> Cr(s) + H2O(I) (unbalanced) How long (in hours) would it take to apply a chromium plating 0.010 mm thick to a car bumper with a surface area of 0.32 m² in an electrolytic cell carrying a current of 25.0 A and assuming electrolysis is 88% efficient? The density of chromium is 7.19 g/cm³. AW of Cr = 52. A. 0.54 h B. 1.25 h C. 2.42 h D. 3.23 h

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...

See similar textbooks

Similar questions

46
Can you help me with HWK3?
12. A typical car/truck battery is a cell made by transferring 2 e- by a reaction between lead and sulfuric acid. If the voltage produced (Eᵒcell) is 12 V, what is AG° of this reaction at 25° C? AG° =
Table 20.1 Half Reaction F2 (g) + 2e7 Cl2 (g) + 2e Br2 (1) + 2e 2C1™ (aq) 2Br (aq) O2 (g) + 4H+ (aq) + 4e¯ Ag (s) → Ag+ e Fe3+ (aq) + e 12 (s) + 2e™ Cu2+ + 2e 2H+ 2e Pb2+ + 2e™ Ni2+ + 2e Lit + e 2F (aq) - Fe2+ (aq) 21 (aq) Cu (s) H2 (8) Pb (s) Ni (s) Li (s) E°(V) +2.87 +1.359 +1.065 2H₂0 (1) +1.23 +0.799 +0.771 +0.536 +0.34 0 -0.126 -0.28 -3.05 21) Using Table 20.1, which substance can oxidize I (aq) to 12 (s)? A) Cu²+ (aq) B) Br (aq) C) Ag (s) D) Br2 (1) E) Ni2+ (aq)
How many moles of Al3+ would be electrolyzed to Al(s) with the same amount of electricity that produces 16.0 g Cu(s) from a solution of Cu(NO3)2?
Shown below are some standard reduction potentials. For which of these compounds is oxidation most favorable? (Imagine you mixed all four of these compounds together in equal quantities. Which one would get oxidized?) a) H2O b) NADH c) O2 d) NAD+
Chromium plating is applied by electrolysis to objects suspended in a dichromate solution, according to this half-reaction: Cr2O7^2- (aq) + H^+ (aq) + e^- —> Cr(s) + H20(l) (unbalanced) How long (in hours) would it take to apply a chromium plating 0.015 mm thick to a car bumper with a surface area of 0.35 m^2 in an electrolytic cell carrying a current of 25.0 A? The density of chromium is 7.19 g/cm^3, AW of Cr = 52.
Be sure to answer all parts. Electrolysis of molten NaCl in a Downs cell is the major isolation step in the production of sodium metal. Assuming that 217 g of Na metal forms, answer the following questions. (a) How many moles of electrons are required? mol e (b) How many coulombs are required? x 100 Enter your answer in scientific notation. (c) How many amps will produce this amount in 9.50 h? A
Balance the following redox reaction in acidic solution, using lowest whole-number coefficients. CIO2 (aq) →CIO2(g) + CI¯(aq) Based on the balanced equation, answer the following questions: The coefficient of CIO2 is: 5 The coefficient of CIO2 is: 3 The coefficient of CI is: 1 The coefficient of H+ is: 4 on the left side of the equation. The coefficient of H2O is: 2 on the right side of the equation.