5.6TheKinetic Molecular Theory of Gases205In this case, the partial pressure of the O2is733 terf=0.964 atmP=733 torr=760 terr/atm0,To find the moles of O2produced, we usev=0.650 LT=22°C+273=295 KR=0.08206 L . atmlK . mol(0.964 atm)(0.650~)n--;;:-;~~~-~-.:..:...::....=.'~-O2 -(0.08206 ~ .aHI1/K •mol)(295K)=2.59 X 10-2molHow many moles of KClO3are required to produce this amount of 02?Use the stoichiometry problem-solving strategy:1~What is the balanced equation?2KCI03(s) ~2KCI(s)+302(g)2 ~What is the mole ratio between KClO3andO2in the balanced equation?1mol HCI2 mol KCI031mol NaHC033mol O23~What are the moles of KClO3?2mol KCI032.59X10-2meI:-02X=1.73X10-2mol KCI033meI:-024 ~What is the mass of KClO3(molar mass122.6g/mol) in the original sample?122.6 g KCIO1.73X10-2~X3=2.12 g KCI031~• Thus the original sample contained 2.12 g KCI03.SEEEXERCISES5.87THROUGH5.895.6~The KineticMoLecuLar Theory of GasesWehave sofar considered the behavior of gases from anexperimental point ofview. Based
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