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Question

Oxygen masks for producing O2\mathrm{O}_2 in emergency situations contain potassium superoxide (KO2)\left(\mathrm{KO}_2\right). It reacts according to this equation:

4 KO2+2 H2O+4 CO24 KHCO3+3 O24\mathrm{~KO}_2+2\mathrm{~H}_2 \mathrm{O}+4\mathrm{~CO}_2\longrightarrow 4\mathrm{~KHCO}_3+3\mathrm{~O}_2

(a) If a person wearing such a mask exhales 0.85 g0.85 \mathrm{~g} of CO2\mathrm{CO}_2 every minute, how many moles of KO2\mathrm{KO}_2 are consumed in 10.010.0 minutes?
(b) How many grams of oxygen are produced in 1.01.0 hour?

Solution

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The formula of the reaction:

4 KO2_2 + 2 H2_2O + 4 CO2_2 \rightarrow 4 KHCO3_3 + 3 O2_2

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