Consider the electrolysis of molten calcium chloride with inert platinum electrodes. The following experimental observations were noted: • Bubbles of pale green chlorine gas are produced at one electrode, Shiny grey molten metallic calcium is produced at the other electrode. Ca2+( )/Ca(s) E° =-2.84 V Cl2(g)/CH() E° = 1.36 V Explain what is happening. Your answer should include the following: • The redox processes happening at each electrode. Justify your choice of oxidation and reduction reactions using oxidation numbers and electron transfer. • Movement of the different identified charges. Relating all the observations to the species concerned. • Balanced half and full equations

Consider the electrolysis of molten calcium chloride with inert platinum electrodes. The following experimental observations were noted: • Bubbles of pale green chlorine gas are produced at one electrode, Shiny grey molten metallic calcium is produced at the other electrode. Ca2+( )/Ca(s) E° =-2.84 V Cl2(g)/CH() E° = 1.36 V Explain what is happening. Your answer should include the following: • The redox processes happening at each electrode. Justify your choice of oxidation and reduction reactions using oxidation numbers and electron transfer. • Movement of the different identified charges. Relating all the observations to the species concerned. • Balanced half and full equations

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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Consider the electrolysis of molten calcium chloride with inert platinum electrodes. The
following experimental observations were noted:
• Bubbles of pale green chlorine gas are produced at one electrode,
Shiny grey molten metallic calcium is produced at the other electrode.
Ca2+( ()/Ca(s)
E° =-2.84 V
Cl2(g)/Cl-(e)
E° = 1.36 V
Explain what is happening. Your answer should include the following:
• The redox processes happening at each electrode.
Justify your choice of oxidation and reduction reactions using oxidation numbers
and electron transfer.
• Movement of the different identified charges.
Relating all the observations to the species concerned.
Balanced half and full equations.
Discussion, with reasons, why this reaction is not spontaneous.

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