Molten NaCI ci | Na 1. Define electrolysis 2. What element is being reduced and oxidized? 3. What electrode pulls the electrons in and electrode that pulls the electrodes out 4. Write the half reaction that occurs in the anode and cathode part of the electrolytic cell

Molten NaCI ci | Na 1. Define electrolysis 2. What element is being reduced and oxidized? 3. What electrode pulls the electrons in and electrode that pulls the electrodes out 4. Write the half reaction that occurs in the anode and cathode part of the electrolytic cell

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

Voltaic or Electrolytic? 1. Balance the reaction if it is spontaneous. 2. Write "no reaction" if it is non-spontaneous cate if the reaction could be used for a voltaic cell or be used in an electrolyt 1. 2 Al(s) + 3CuCla(aq) → Circle one: VOLTAIC/ELECTROLYTIC Substance oxidized: Substance reduced: 2. Pb(s) + Al(NO:):(aq) > Circle one: VOLTAIC / ELECTROLYTIC
Which of the following is a true statement regarding an electrolytic cell? Oxidation occurs at the cathode. Electrons flow from the cathode to the anode. All these statements are true. Electrical energy is used to cause a chemical reaction to occur that would be otherwise be nonspontaneous.
What is a fuel cell? What is the most common type of fuel cell and what reactions occur at its anode and cathode?
Which statement is true a. Galvanic cells involve non-spontaneous redox reactions b. The oxidizing agents give off electrons C. In chemical cells the electrons flow from cathode to anode d. Electrolytic cells need an external source of electricity to proceed
2. The reduction of aluminum ions occurs as: Al³+ (aq) + 3e → Al(s) After applying a certain amount of current through an electrolytic cell, 0.1328 g of aluminum is deposited at the electrode a. How many moles of aluminum metal has been deposited? b.How many aluminum atoms have been deposited? (Use Avogadro's number). c. How many electrons were required for the reduction of this much aluminum? d. If the electronic charge is 1.60 x 10-¹C, what is the total electrical charge used? e. If a constant current of 90 mA were applied, what was the time elapsed in seconds and in minutes?
How is the amount of current flowing through an electrolytic cell related to the amount of product produced in the redox reaction? Match the items in the left column to the appropriate blanks in the sentences on the right. multiplied coulombs Avogadro's 1 mol Faraday's 1g ampers 6.022 x 10¹ mol volts divided The number of moles of electrons that have flowed in a given electrolysis cell can be determined by measuring the total charge that has flowed through the cell. If the amount of current flowing through the cell is by the time that the current flowed, the total charge that passed through the cell in that time can be found. The relationship between charge and the number of moles of electrons constant, which corresponds to the charge in is given by of of electrons. These relationships are used to solve problems involving the stoichiometry of electrolytic cells. Reset Help
8. The electrolysis of copper (II) sulfate using carbon electrodes is demonstrated to a chemistry class. In the demonstration, a 1.50 A current passes through 75.0 mL of 0.125 mol/1. copper (II) sulfate solution. How long, in minutes, would it take to plate all of the copper from the solution?
Cu
PART 2: Answer what is asked for each problem and show your solution. Round your answers to four decimal places and they must be enclosed all in a box. 1. Given the following reduction potentials: Ag*(aq) + e → Ag(s) Zn?"(aq) + 2e → Zn(s) Calculate the cell potential for the following reaction and predict whether the reaction will take place. If it will take place write the cell notation. Znº"(aq) + 2Ag(s)→ Zn(s) + 2Ag*(aq) E° = 0.80 V; E° = -0.76 V 2. A chromium metal was deposited coming from a solution of Cr*³. The amount of the said metal deposited weighs 2.19 g. The process is made possible through a current of 35.2 Amperes in electrolyte cell. Determine the following: a. How much charge (in C) is required? b. How long (in min) would it take for the reaction to occur?
Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. - a Fe electrode in 1.0 M FeCl solution - a Ni electrode in 1.0 M Ni(NO) solution When the cell is running spontaneously, which of the choices are true? a.) The nickel electrode gains mass and the nickel electrode is the cathode. b.) The nickel electrode loses mass and the nickel electrode is the cathode. c.) The iron electrode gains mass and the iron electrode is the anode. d.)The iron electrode loses mass and the iron electrode is the cathode.
A rod made of an unknown metal, M, is dipped into a solution containing both X2+ and Z2+ cations. q1: Will a reaction occur when the rod is dipped into the solution? And if so what solid will begin to form? q2: If you were to create a voltaic cell using M, which (single) metal would you put as the cathode and anode, respectively? q3: f Z is Zinc, identify metals X and M
Which cell is generally used in hearing aids?Name the material of the anode,cathode and the electrolyte. Write the reactions involved.