Oxygen masks for producing O2 in emergency situation contains potassium superoxide (KO2). The chemical reaction for reaction of K2O to produce O2 is shown below. 4 KO2 + 2 H2O + 4 CO2 → 4 KHCO3 + 3 O2 (A) if a person wearing such a mask exhales 0.65g of CO2 every minute, then how many moles of KO2 will be consumed in 15 minutes. (B) calculate the number of grams of O2 that will be produced in 15 minutes.
Oxygen masks for producing O2 in emergency situation contains potassium superoxide (KO2). The chemical reaction for reaction of K2O to produce O2 is shown below. 4 KO2 + 2 H2O + 4 CO2 → 4 KHCO3 + 3 O2 (A) if a person wearing such a mask exhales 0.65g of CO2 every minute, then how many moles of KO2 will be consumed in 15 minutes. (B) calculate the number of grams of O2 that will be produced in 15 minutes.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter3: Equation, The Mole, And Chemical Formulas
Section: Chapter Questions
Problem 3.49QE:
One of the ways to remove nitrogen monoxide gas, a serious source of air pollution, from smokestack...
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Oxygen masks for producing O2 in emergency situation contains potassium superoxide (KO2). The
4 KO2 + 2 H2O + 4 CO2 → 4 KHCO3 + 3 O2
(A) if a person wearing such a mask exhales 0.65g of CO2 every minute, then how many moles of KO2 will be consumed in 15 minutes.
(B) calculate the number of grams of O2 that will be produced in 15 minutes.
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