As explained in the book, the Voltaic cell is where the two components of a spontaneous redox reaction are separated by an electric circuit. The electrons being transferred travel through the electric circuit, and their kinetic energy can thus be utilized by devices such as a light. a. Note the half-reaction on the oxidation side. As the electron is taken away through the electric circuit, what is left? Which component of the salt bridge (the cation, Na*, or the anion, Cl") will migrate towards this side to balance the charges? As shown on the figure, the electrode where oxidation is taking place is called the b. Now note the half-reaction on the reduction side. As the electron arrives from the electric circuit, what does it consume? Which component of the salt bridge (the cation, Na*, or the anion, Cl) will migrate towards this side to balance the charges? As shown on the figure, the electrode where reduction is taking place is called the c. What is the direction of the electron flow through the external electric circuit? The electrons flow from the to the

As explained in the book, the Voltaic cell is where the two components of a spontaneous redox reaction are separated by an electric circuit. The electrons being transferred travel through the electric circuit, and their kinetic energy can thus be utilized by devices such as a light. a. Note the half-reaction on the oxidation side. As the electron is taken away through the electric circuit, what is left? Which component of the salt bridge (the cation, Na, or the anion, Cl") will migrate towards this side to balance the charges? As shown on the figure, the electrode where oxidation is taking place is called the b. Now note the half-reaction on the reduction side. As the electron arrives from the electric circuit, what does it consume? Which component of the salt bridge (the cation, Na, or the anion, Cl) will migrate towards this side to balance the charges? As shown on the figure, the electrode where reduction is taking place is called the c. What is the direction of the electron flow through the external electric circuit? The electrons flow from the to the

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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You are choosing two metals that will show electrons moving from the right to the left. Please be specific. The pretending image is the the image you will use to pick your metals. The image with the blue background is there for help when writing macroscopic observations and half-reactions (add the zero to your half-reactions when needed).
19. The following choices are primary batteries, along with their metal electrodes stated in parenthesis. Which of the following primary batteries will produce the most electrical energy if all the batteries stated are used for an hour? You can refer to the electrochemical series to determine the number of electrons produced by the metal substance. Assume all half-cell reactions are spontaneous. a. Aluminum-zinc battery b. Calcium-lead battery, c. Potassium-sodium battery d. Calcium-zinc battery
What happens at the anode in the voltaic cell? 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
If the given statement is true, write T. Otherwise, write F and explain why it is false 1)An electrolytic cell is used to generate electricity from chemical reactions 2) The reactant and the product need to have equal concentrations for a chemical reaction to be in equilibrium.
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
Represent in the conventional manner, i.e., anode/cathode, the voltaic cell in which each of the following reactions occur spontaneously. B. 2Al + 3Cl2 --> 2AlCl3
A student mistakenly puts the opposite reactants into a voltaic cell, then uses a voltmeter to measure the voltage. What will happen? There could be sparks flying and possible fire or worse. No reaction will happen. The student may experience an electrical shock. The measured voltage will be negative.