Dalton’s Law of Partial Pressures/Effusion 1.Calculate and use the pressure in torr. 2.Determine the partial pressure of the light molecules. 3.Determine.

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Presentation transcript:

Dalton’s Law of Partial Pressures/Effusion 1.Calculate and use the pressure in torr. 2.Determine the partial pressure of the light molecules. 3.Determine the partial pressure of the light molecules. 4.Calculate the partial pressure of the heavy molecules.

Dalton’s Law of Partial Pressures/Effusion A chemist collects O 2 over H 2 O using the reaction: 2 KClO 3 → 2 KCl + 3 O 2 The experiment is shown right. The total pressure In the bottle is 745 mmHg, T = 30 o C, and the total volume (O 2 & H 2 O)is 371 mL. 1..Write the partial pressure (vapor pressure) of H 2 O at 30 o C. ANS: VP = 32 torr (mmHg) See, for example Tro page table Calculate the moles of H 2 O. ANS = 6.28 X mol 3. Calculate the partial pressure of O 2. ANS = 713 torr 4. Calculate the moles of O 2. ANS = mol 5. Which molecule has the greatest velocity? Show effusion from slide 1.

Dalton’s Law of Partial Pressures A chemist collects O 2 over H 2 O. P total = atm, T = 35 o C, and V total = 521 mL. The vapor pressure of water at 35 o C is 42 torr. [Tro page table 5.4]. 1.Calculate the vapor pressure of water in atm. ANS: atm 2. Calculate the partial pressure of O 2. ANS: atm 3. Calculate the moles of O 2. ANS: mol

Dalton’s Law of Partial Pressures A chemist has a gas sample (P total = 1.24 atm) consisting of 0.61 mol of He and 2.77 mol of Ne. Calculate the partial pressures of He and Ne. ANS: P He = 0.22 atm P Ne = 1.02 atm