1. A voltaic cell consists of two half-cells. One of the half-cells contains a platinum electrode surrounded by chromium (III) and dichromate ions. The other half-cell contains a platinum electrode surrounded by bromate ions and liquid bromine. Assume that the cell reaction, which produces a positive voltage, involves both chromium (III) and bromate ions. The cell is at 25°C. Information for the bromate reduction half reaction is as follows: 12H*(aq) + 10e- – Br,(1) + 6H,0 E = 1.478 V (a) Write the cell diagram notation (b) Calculate E for the cell (c) Calculate the voltage of the cell when all ionic species except H+ are 0.1500M and the pH is at -0.301. 2. Consider a voltaic cell at 25°C in which the following reaction takes place. 30,(g) + 4NO(g) + 2H2O→ 4NO, (aq) + 4H*(ag) (a) Calculate E for the cell (b) Calculate E under the following conditions: [NO,] = 0.750 M, PNO = 0.993 atm, Po, = 0.515 atm, pH = 2.85. 3. A metallurgist wants to goldplate a thin sheet with the following dimensions: 1.5 in. x 8.5 in. x 0.0012 in. The gold plating must be 0.0020 in. thick. (a) How many grams of gold (p = 19.3 g/cm²) are required? (b) How long will it take to place the sheet from AUCN using a current of 7.00 A? Assume 85% efficiency.
1. A voltaic cell consists of two half-cells. One of the half-cells contains a platinum electrode surrounded by chromium (III) and dichromate ions. The other half-cell contains a platinum electrode surrounded by bromate ions and liquid bromine. Assume that the cell reaction, which produces a positive voltage, involves both chromium (III) and bromate ions. The cell is at 25°C. Information for the bromate reduction half reaction is as follows: 12H*(aq) + 10e- – Br,(1) + 6H,0 E = 1.478 V (a) Write the cell diagram notation (b) Calculate E for the cell (c) Calculate the voltage of the cell when all ionic species except H+ are 0.1500M and the pH is at -0.301. 2. Consider a voltaic cell at 25°C in which the following reaction takes place. 30,(g) + 4NO(g) + 2H2O→ 4NO, (aq) + 4H*(ag) (a) Calculate E for the cell (b) Calculate E under the following conditions: [NO,] = 0.750 M, PNO = 0.993 atm, Po, = 0.515 atm, pH = 2.85. 3. A metallurgist wants to goldplate a thin sheet with the following dimensions: 1.5 in. x 8.5 in. x 0.0012 in. The gold plating must be 0.0020 in. thick. (a) How many grams of gold (p = 19.3 g/cm²) are required? (b) How long will it take to place the sheet from AUCN using a current of 7.00 A? Assume 85% efficiency.
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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![1. A voltaic cell consists of two half-cells. One of the half-cells contains a platinum electrode surrounded
by chromium (III) and dichromate ions. The other half-cell contains a platinum electrode surrounded by
bromate ions and liquid bromine. Assume that the cell reaction, which produces a positive voltage,
involves both chromium (III) and bromate ions. The cell is at 25°C. Information for the bromate reduction
half reaction is as follows:
2BFO, -(ag) + 12н*(ад) + 10ет — Brz() + 6H,0
Ed = 1.478 y
(a) Write the cell diagram notation
(b) Calculate E° for the cell
(c) Calculate the voltage of the cell when all onic species except H+ are 0.1500M and the pH is at -0.301.
2. Consider a voltaic cell at 25°C in which the following reaction takes place.
302(g) + 4NO(g) + 2H¿O→ 4NO, (aq) + 4H†(aq)
(a) Calculate E° for the cell
(b) Calculate E under the following conditions: [NO,] = 0.750 M, PNo = 0.993 atm, Po, = 0.515 atm, pH =
2.85.
3. A metallurgist wants to goldplate a thin sheet with the following dimensions: 1.5 in. x 8.5 in. x 0.0012
in. The gold plating must be 0.0020 in. thick.
(a) How many grams of gold (p = 19.3 g/cm³) are required?
(b) How long will it take to place the sheet from AuCN using a current of 7.00 A? Assume 85% efficiency.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc008a07d-8ee8-487c-b6c3-47f065225819%2F488abbcc-dade-4cea-86cf-43274da4f4af%2Fr6cedt_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1. A voltaic cell consists of two half-cells. One of the half-cells contains a platinum electrode surrounded
by chromium (III) and dichromate ions. The other half-cell contains a platinum electrode surrounded by
bromate ions and liquid bromine. Assume that the cell reaction, which produces a positive voltage,
involves both chromium (III) and bromate ions. The cell is at 25°C. Information for the bromate reduction
half reaction is as follows:
2BFO, -(ag) + 12н*(ад) + 10ет — Brz() + 6H,0
Ed = 1.478 y
(a) Write the cell diagram notation
(b) Calculate E° for the cell
(c) Calculate the voltage of the cell when all onic species except H+ are 0.1500M and the pH is at -0.301.
2. Consider a voltaic cell at 25°C in which the following reaction takes place.
302(g) + 4NO(g) + 2H¿O→ 4NO, (aq) + 4H†(aq)
(a) Calculate E° for the cell
(b) Calculate E under the following conditions: [NO,] = 0.750 M, PNo = 0.993 atm, Po, = 0.515 atm, pH =
2.85.
3. A metallurgist wants to goldplate a thin sheet with the following dimensions: 1.5 in. x 8.5 in. x 0.0012
in. The gold plating must be 0.0020 in. thick.
(a) How many grams of gold (p = 19.3 g/cm³) are required?
(b) How long will it take to place the sheet from AuCN using a current of 7.00 A? Assume 85% efficiency.
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