Partial Pressure.

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Presentation transcript:

Partial Pressure

Dalton’s Law of Partial Pressures V and T are constant P2 Ptotal = P1 + P2 P1

PA = nART V PB = nBRT V XA = nA nA + nB XB = nB nA + nB PT = PA + PB Consider a case in which two gases, A and B, are in a container of volume V. PA = nART V nA is the number of moles of A PB = nBRT V nB is the number of moles of B XA = nA nA + nB XB = nB nA + nB PT = PA + PB PA = XA PT PB = XB PT Pi = Xi PT mole fraction (Xi ) = ni nT

A mixture of gases contains 4. 46 moles of neon (Ne), 0 A mixture of gases contains 4.46 moles of neon (Ne), 0.74 mole of argon (Ar), and 2.15 moles of xenon (Xe). Calculate the partial pressures of the gases if the total pressure is 2.00 atm at a certain temperature.

Collecting a Gas over Water ?????? 2KClO3 (s) 2KCl (s) + 3O2 (g) PT = PO + PH O 2

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5.15 Oxygen gas generated by the decomposition of potassium chlorate is collected as shown in slide 7. The volume of oxygen collected at 24°C and atmospheric pressure of 762 mmHg is 128 mL. Calculate the mass (in grams) of oxygen gas obtained. The pressure of the water vapor at 24°C is 22.4 mmHg.