Potassium superoxide, KO2, is often used in oxygen masks(such as those used by firefighters) because KO2 reacts withCO2 to release molecular oxygen. Experiments indicate that 2mol of KO2(s) react with each mole of CO2(g). (a) The productsof the reaction are K2CO3(s) and O2(g). Write a balanced equationfor the reaction between KO2(s) and CO2(g). (b) Indicatethe oxidation number for each atom involved in the reactionin part (a). What elements are being oxidized and reduced?(c) What mass of KO2(s2) is needed to consume 18.0 g CO2(g)?What mass of O2(g) is produced during this reaction?
Potassium superoxide, KO2, is often used in oxygen masks(such as those used by firefighters) because KO2 reacts withCO2 to release molecular oxygen. Experiments indicate that 2mol of KO2(s) react with each mole of CO2(g). (a) The productsof the reaction are K2CO3(s) and O2(g). Write a balanced equationfor the reaction between KO2(s) and CO2(g). (b) Indicatethe oxidation number for each atom involved in the reactionin part (a). What elements are being oxidized and reduced?(c) What mass of KO2(s2) is needed to consume 18.0 g CO2(g)?What mass of O2(g) is produced during this reaction?
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
Chapter20: The Representative Elements
Section: Chapter Questions
Problem 119IP: While selenic acid has the formula H2SeO4 and thus is directly related to sulfuric acid, telluric...
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Question
Potassium superoxide, KO2, is often used in oxygen masks
(such as those used by firefighters) because KO2 reacts with
CO2 to release molecular oxygen. Experiments indicate that 2
mol of KO2(s) react with each mole of CO2(g). (a) The products
of the reaction are K2CO3(s) and O2(g). Write a balanced equation
for the reaction between KO2(s) and CO2(g). (b) Indicate
the oxidation number for each atom involved in the reaction
in part (a). What elements are being oxidized and reduced?
(c) What mass of KO2(s2) is needed to consume 18.0 g CO2(g)?
What mass of O2(g) is produced during this reaction?
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