What is the primary difference between a voltaic and an electrolytic cell? Voltaic cells are used only in laboratories; electrolytic cells are used only in industrial applications. .a O The electrolytic cell can be used as a power supply; the voltaic cell must itself have power supplied in order to .b O function. The voltaic cell is a real reaction that is used in everyday applications; the electrolytic cell is a theoretical reaction .c O that does not have any real-life applications. The reaction in a voltaic cell is exothermic; the one in an electrolytic cell is endothermic. .d O The reaction in a voltaic cell is spontaneous; the one in an electrolytic cell is nonspontaneous. .e O

What is the primary difference between a voltaic and an electrolytic cell? Voltaic cells are used only in laboratories; electrolytic cells are used only in industrial applications. .a O The electrolytic cell can be used as a power supply; the voltaic cell must itself have power supplied in order to .b O function. The voltaic cell is a real reaction that is used in everyday applications; the electrolytic cell is a theoretical reaction .c O that does not have any real-life applications. The reaction in a voltaic cell is exothermic; the one in an electrolytic cell is endothermic. .d O The reaction in a voltaic cell is spontaneous; the one in an electrolytic cell is nonspontaneous. .e O

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

A layer of chromium is electroplated on an automobile bumper by passing a constant current of 40.0 A through a cell that contains Cr3+(aq). How many hours are required to deposit 151 g of chromium? Note: Electroplating is the formation of a metal by the reduction of a metal cation. Select one: a. 32.7 h b. 58.4 h c. 5.84 h d. 3.27 h e. 19.5 h f. 1.95 h
Danial cell is an example of .A Concentration cell .B Galvanic cell .C Electrolytic cell .D none
The flow of e- in an electrochemical cell is always from to O anode, cathode O cathode, anode O cathode, electrode .electrode, anode
14, Table 1 below shows information about three simple voltaic cells. Pair of metals W and X X and Y W and Z Potential difference (V) Positive terminal 0.7 X 2.0 Y 1.6 Calculate the potential difference of a voltaic cell which uses Y and Z as electrodes. A. 0.4 V B. 0.9 V C. 1.1 V D. 1.3 V
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.
Which of the following statements is(are) true for all galvanic cells? 1. Reduction occurs at the cathode. II. The anode gains mass during discharge (note: this means operation of the cell.) III. The voltage is less than or equal to zero. O only I O only III O only II O L I, and II O Il and II
An electrochemical cell has a positive standard cell potential but a negative cell potential. Which statement is true? a. K> 1; Q > K b. K K c. K> 1; Q < K d. K< 1; Q< K
1) Construct a zinc-copper electrochemical cell using 1.0 M Zn2+ and 1.0 M Ni2+ solutions. a. Provide the shorthand notation. b. What is the EMF of this cell (include units)? c. For the voltage that you are measuring, is this E°cell or Ecell? Explain.
06. Show Solutions
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.
‏choose the best answer
Please explain step by step. ** Electrolysis 4. Sketch a cell for the electrolysis of aqueous HCl using copper elec trodes. Label the anode and cathode and give the electrode reactions. Indicate the directions in which the electrons and ions move and the connections to the terminal of the voltage source.