Kll (Part-I)s passedCalculateNTP.passingILine)on-theElectrochemistryorExample 9. In an electrolysis experiment, a current waspassed for 5 hours through two cells connected in series. The firstcell contains a solution of gold salt and the second cell containscopper sulphate solution. 9.85 g of gold was deposited in the firstcell. If the oxidation number of gold is +3, find the amount of cop-per deposited on the cathode in the second cell. Also, calculate themagnitude of the current in ampere.Solution: We know that,Mass of Au deposited Eq. mass of AuMass of Cu deposited Eq. mass of Cu=Eq. mass of Au=- ; Eq. mass of Cu = 63.519732Mass of copper deposited63.53= 9.85 xg= 4.7625 g197Let Z be the electrochemical equivalent of Cu.E=ZX 96500orZ=E63.596500 2 × 96500Applying W = Z xixtt = 5 hours = 5 x 3600 second4.7625=63.5-xix5x36002 × 96500ori=4.7625 × 2 × 9650063.5x5x3600= 0.804 ampereExample 10. How long has a current of 3 ampere to be ap-plied through a solution of silver nitrate to coat a metal surface of80 cm with 0.005 mm thick layer? Density of silver is10.5 g cm-30.42 × 96500108 x 3Example 11.What currentquired to liberate 10 g of chlorineone hour?Solution: Applying E=Z=35.5=Z-orZ==Now, applying the formulaW=Z:where, W = 10 g.2= 359610:i=35.Example 12. 0.2964 g ofa current of 0.5 ampere for 30per sulphate. Calculate the an(1 faraday=96500 coulomb)Solution: Quantity of ch=0.5x30x900 coulomb deposit copp96500 coulomb deposit cThus, 31.78 is the equivaAt. mass=Example 13. Calculatebe required to reduce 12.3rent efficiency for the proce

Since you have asked multiple question, we will solve the first question for you. If you want any…

Example 9. In an electrolysis experiment, a current was passed for 5 hours through two cells connected in series. The first cell contains a solution of gold salt and the second cell contains copper sulphate solution. 9.85 g of gold was deposited in the first cell. If the oxidation number of gold is +3, find the amount of cop- per deposited on the cathode in the second cell. Also, calculate the magnitude of the current in ampere. Solution: We know that,

Example 9. In an electrolysis experiment, a current was passed for 5 hours through two cells connected in series. The first cell contains a solution of gold salt and the second cell contains copper sulphate solution. 9.85 g of gold was deposited in the first cell. If the oxidation number of gold is +3, find the amount of cop- per deposited on the cathode in the second cell. Also, calculate the magnitude of the current in ampere. Solution: We know that,

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

Calculate the concentration of an unknown solution in a concentration cell. A concentration cell consisting of two hydrogen electrodes (P H2- latm), where the cathode is a standard hydrogen electrode and the anode solution has an unknown pH, has a cell voltage of 0.193 V. What is the pH in the unknown solution? Assume the temperature of the solutions is 298 K. !! pH =
1.How many grams of NaCl is present on 5.0 mL of 1.0 % m/V NaCl solution? 2. A zinc bar weighing 3.0 kg is attached to a buried iron pipe to protect the pipe from corrosion. An average current of 0.020 A flows between the bar and the pipe. How many years will be required for the zinc bar to be entirely consumed?
A certain half-reaction has a standard reduction potential Ered = -1.01 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 1.00 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used…
Element A has a standard reduction potential of +0.74V, whereas Element B has a standard reduction potential of -1.15V. Which of the following statements is correct with respect to building a Galvanic cell with these two elements? A. A will be the cathode, B will be the anode, and the cell potential will be positive. B. A will be the cathode, B will be the anode, and the cell potential will be negative. C. A will be the anode, B will be the cathode, and the cell potential will be positive. D. A will be the anode, B will be the cathode, and the cell potential will be negative. E. The anode, cathode, and cell potential must all be experimentally determined.
A certain half-reaction has a standard reduction potential E=+1.34 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.20 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer reguires this half-reaction to happen at the anode of the cell. nh Data Half-Reaction E° (V) 0.7996 Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? = Ov Ag+ (aq) + e- -→ Ag (s) O yes, there is a minimum. E %3D red Al3+ (aq) + 3e- → Al (s) -1.676 1.692 Au+ (aq) + e → Au (s) If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. O no minimum Au3+ (aq) + 3e- → Au (s) 1.498 Ba2+ (ag) + 2e- - Ba (s) -2.912 Brz (1) + 2e 2Br (aq) 1.066 - Ca2+ (ag) + 2e Ca (s) -2.868 Is there a maximum standard reduction potential that the half-reaction used at the…
Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used at the anode of this cell. Note: write the half reaction as it would actually occur at the anode. Oyes, there is a minimum. no minimum yes, there is a maximum. no maximum 0 E 0V red 0 E red = = ☐v
Sometimes in a galvanic cell, an inert electrode is needed. What element is typically used? (Give the symbol)
3.A technician is plating a faucet with 1.26 g of Cr from an electrolytic bath containing aqueous Cr2(SO4)3. If 18.5 min is allowed for the plating, what current is needed? Faraday's constant = 96, 485 C/mol . Molar mass Ni = 51.9961 g/mol Group of answer choices 2.10A 1.36A 3.16A 6.31A
It is known that at both electrodes of the voltaic cell there is an acid solution that produces hydrogen gas at the anode and cathode. The flow of electrons flows from a concentration of 0.05 M to a higher concentration of 0.5 M. If the rods at the anode and cathode are platinum (Pt), then the voltaic cell potential measured on the voltmeter is ... A. 0.5092 V B. 0.1184 V C. 0.1776 V D. 0.0592 V