During the electrolysis of aqueous KCI solution using inert electrodes, gaseous hydrogen is evolved at one electrode and gaseous chlorine at the other electrode. The solution around the electrode at which hydrogen gas is evolved becomes basic as the electrolysis proceeds. Which of the following responses describe or are applicable to the cathode and the ?reaction that occurs at the cathode the negative electrode (2) the positive electrode (1) "Cl2 + 2 e - 2 CI (4) "cr - Cl2 + 2 e 2 (3) "H20 + 2 e- H2 + 2 OH 2 (6) "H20 – 02 + 4 H* + 4 e 2 (5) electrons flow into the electrode (8) electrons flow from the electrode to (7) the external circuit from the external circuit reduction (10) oxidation (9)

During the electrolysis of aqueous KCI solution using inert electrodes, gaseous hydrogen is evolved at one electrode and gaseous chlorine at the other electrode. The solution around the electrode at which hydrogen gas is evolved becomes basic as the electrolysis proceeds. Which of the following responses describe or are applicable to the cathode and the ?reaction that occurs at the cathode the negative electrode (2) the positive electrode (1) "Cl2 + 2 e - 2 CI (4) "cr - Cl2 + 2 e 2 (3) "H20 + 2 e- H2 + 2 OH 2 (6) "H20 – 02 + 4 H* + 4 e 2 (5) electrons flow into the electrode (8) electrons flow from the electrode to (7) the external circuit from the external circuit reduction (10) oxidation (9)

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

In the electrolysis of a 200 mL unknown metal solution, 0.0434 grams of cathode mass increases when a current of 0.50 A is passed through the cell for 5 minutes. Other experiments reveal that the metal has +2 valence. Which of the following is the metal in the electrolysis solution? (Pt: 195 g/mol; Si: 28,08 g/mol; Fe: 55,8 g/mol; Cd: 112,4 g/mol; Mn: 54,94 g/mol; 1 F : 96485 C)
75. Which of the following statements associated with the pH meter is incorrect? (A) The pH meter should include a working electrode, a reference electrode, and a counter electrode. (B) The pH meter is unable to determine the pH of 0.1 M NaOH. (C) Silver chloride-coated silver wire is commonly used as a reference electrode in the pH meter. (D) The glass membrane must be hydrated. (E) The difference in potential between the inner and outer layers is the boundary potential.
If an electrolysis plant operates its electrolytic cells at a total current of 150. A, how long , (in hours) will it take to produce 2.0 Ibs of Mg(s) from seawater containing Mg2+? (1 faraday = 96,485 coulombs) hr
Q26 (A). Define an electrolytic cell. Describe with a neat diagram, an electrolytic cell for the decomposition of molten NaCl. Write the reactions at the anode and cathode
Write the anodic and cathodic half-reactions that take place when a piece of galvanized steel is corroded in an acidic medium (pH = 4.5).
How long would it take to deposit 7.54 g of copper (molar mass 63.55 g/mol) at the cathode of an electrolytic cell, if a current of 15.9 A is passed through an aqueous solution of CuSOa? 19.4 min 32.2 min 24.0 min 33.9 min 26.8 min
A copper rod was purified by using it as the anode in the electrolysis of a 1.0 M copper (II) sulphate solution. The cathode was made of pure copper. The mass of the cathode before the electrolysis was 0.52 g. After the electrolysis, mass of the cathode was 1.75 g. a. If the current used was 1.5 A, for how many minutes was the electrolysis performed? b. Calculate the magnitude of the current that must be used so that the time of electrolysis can be shortened to 20 minutes.
6) Calculate the potential of a cell, Eºcell, made with a standard bromine electrode as the anode and a standard chlorine electrode as the cathode. Write the shorthand cell notation.
How long (in hours) must a current of 5.0 amperes be maintained to electroplate 60g of calcium from molten CaCl2?
what mass, in g, of copper will be deposited from a solution of Cu^2+ by a current of 2.43 A in 7.52 h?
How long would it take to deposit 9.38 g of copper (molar mass 63.55 g/mol) at the cathode of an electrolytic cell, if a current of 23.2 A is passed through an aqueous solution of CUSO4?
write the half-reactions that occur at the anode and cathode during the electrolysis of NH4Cl in aqueous solution.