Activity 3: Practical uses of electrochemistry The principles of cells are used to make electrical batteries. In science, a battery is a device that stores chemical energy and make it available in electrical forms. Batteries are made up of electrochemical devices such as one or more galvanic cells or fuel cell. Enumerate the different uses of electrochemistry in different field of specialization. Write your answers on the space provided. 1. Science and technology 2. Economics 3. Health

Activity 3: Practical uses of electrochemistry The principles of cells are used to make electrical batteries. In science, a battery is a device that stores chemical energy and make it available in electrical forms. Batteries are made up of electrochemical devices such as one or more galvanic cells or fuel cell. Enumerate the different uses of electrochemistry in different field of specialization. Write your answers on the space provided. 1. Science and technology 2. Economics 3. Health

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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1. Draw a diagram that shows a battery made of three galvanic cells. How does the voltage of the battery compare with the voltage of its cells? | ©
232. Subject :- Chemistry
11- An electrolytic cell is set up using inert electrodes in an aqueous copper(II) sulfate solution. After an hour of electrolysis, the solution is tested. The concentration of copper(II) ions has decreased, while the concentration of hydrogen ions has increased. The mass of one electrode has also increased. Explain these observations using the half-reaction equation for each electrode.
1) How are the terms “electrochemical cell” and “battery” related? 2) Give a brief description of how and why a battery works. 3) There are two types of batteries: Primary and secondary. How are these types of batteries different from one another? How are they the same?
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AGº. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E". His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. calculated quantities (Check the box next to any that are wrong.) cell n aG K E -21 1.42 x 10 A 1 119. kJ/mol O 1.23 V -- В - 51. kJ/mol 1.16 X 10 -0.53 V -11 2.06 X 10 1 -61. kJ/mol 0.63 V
Which statement about electrolytic cells is false? Electrolytic cells convert electrical energy into chemical energy. O The redox reaction is non-spontaneous. The anode and cathode are placed in the same container with the aqueous electrolyte. O The anode is negative and the cathode is positive. O The external battery supplies the electrons.