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# Scan_Doc0113 - 5.6 The Kinetic Molecular Theory of Gases...

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5.6 TheKinetic Molecular Theory of Gases 205 In this case, the partial pressure of the O 2 is 733 terf = 0.964 atm P = 733 torr = 760 terr/atm 0, To find the moles of O 2 produced, we use v = 0.650 L T = 22°C + 273 = 295 K R = 0.08206 L . atmlK . mol (0.964 atm)(0.650~) n - -;;:-;~~~-~-.:..:...:: .... =.'~- O 2 - (0.08206 ~ . aHI1/K • mol)(295 K) = 2.59 X 10- 2 mol How many moles of KClO 3 are required to produce this amount of 02? Use the stoichiometry problem-solving strategy: 1~ What is the balanced equation? 2KCI0 3 (s) ~ 2KCI(s) + 30 2 (g) 2 ~ What is the mole ratio between KClO 3 and O 2 in the balanced equation? 1mol HCI 2 mol KCI0 3 1mol NaHC0 3 3mol O 2 3~ What are the moles of KClO 3 ? 2mol KCI0 3 2.59 X 10- 2 meI:-02 X = 1.73 X 10- 2 mol KCI0 3 3meI:-02 4 ~ What is the mass of KClO 3 (molar mass 122.6 g/mol) in the original sample? 122.6 g KCIO 1.73 X 10- 2 ~ X 3 = 2.12 g KCI0 3 1~ • Thus the original sample contained 2.12 g KCI0 3 . SEE EXERCISES 5.87 THROUGH 5.89 5.6~ The Kinetic MoLecuLar Theory of Gases Wehave sofar considered the behavior of gases from anexperimental point ofview. Based
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