A current of 14.2A is passed through an electrolysis cell containing molten CaCl₂ for 37.0 minutes. (a) Predict the products of the electrolysis and write the reactions occurring at the anode and cathode. Write electrons as e. Use smallest integer coefficients possible and omit states. If a box is not needed, leave it blank. Cathode reaction: Ca2+ + 2e Anode reaction: + 2C1 1 Ca(1) 1 Cl₂(g) + + 2e
A current of 14.2A is passed through an electrolysis cell containing molten CaCl₂ for 37.0 minutes. (a) Predict the products of the electrolysis and write the reactions occurring at the anode and cathode. Write electrons as e. Use smallest integer coefficients possible and omit states. If a box is not needed, leave it blank. Cathode reaction: Ca2+ + 2e Anode reaction: + 2C1 1 Ca(1) 1 Cl₂(g) + + 2e
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 84QAP: Calcium metal can be obtained by the direct electrolysis of molten CaCl2, at a voltage of 3.2 V. (a)...
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Transcribed Image Text:Calculate quantity of materials produced from the electrolysis of a molten salt.
A current of 14.2A is passed through an electrolysis cell containing molten CaCl, for 37.0 minutes.
(a) Predict the products of the electrolysis and write the reactions occurring at the anode and cathode. Write electrons
as e. Use smallest integer coefficients possible and omit states. If a box is not needed, leave it blank.
Cathode reaction:
Ca²+
Anode reaction:
+
2e
Formed at anode:
2C1-
- Ca(1)
1 Cl₂(g)
(b) Calculate the grams of metal or liters of gas formed at the cathode and anode (assume gases are at 298 K and
1.00 atm).
Formed at cathode:
grams
+ 2e
liters
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