Oxygen masks for producing O2 in emergency situations contain potassium superoxide (KO2). It reacts according to the following equation: 4 KO2 + 2 H20 + 4 CO2 → 4 KHCO3+ 302 (a) If a person wearing such a mask exhales 0.85 g of CO, every minute, how many moles of KO, are consumed in 10.0 minutes? i mol KO2 (b) How many grams of oxygen are produced in 1.0 hour? i g O2

Oxygen masks for producing O2 in emergency situations contain potassium superoxide (KO2). It reacts according to the following equation: 4 KO2 + 2 H20 + 4 CO2 → 4 KHCO3+ 302 (a) If a person wearing such a mask exhales 0.85 g of CO, every minute, how many moles of KO, are consumed in 10.0 minutes? i mol KO2 (b) How many grams of oxygen are produced in 1.0 hour? i g O2

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 59QRT: Nitrogen monoxide is oxidized in air to give brown nitrogen dioxide. Starting with 2.2 mol NO,...

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