Before you solve these problems , you can read this subject for Dalton’s Law of Partial Pressures (Statement, Mathematical,Importance, Application).
Problem (2): Calculate the total number of moles in a 10.5-L sample of gas at 292 K, containing O2 at 0.622 atm and N2 at 0.517 atm. Also calculate the number of moles of present.
Problem (3): Oxygen gas is collected over water in an apparatus such as that shown in Figure 12.8 at a barometric pressure of 759 torr at 23 oC
Problem (4): What volume of oxygen, collected over water, will be obtained at 23 oC and 762 torr barometric pressure from the thermal decomposition of 0.0600 mol of KClO3
Problem (5): 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.
(1.21 + 0.20 + 0.586) atm = 2.00 atm.
Problem (6): Oxygen gas generated by the decomposition of potassium chlorate is collected as shown in Figure (1). 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.
The density of the oxygen gas is (0.164 g/0.128 L), or 1.28 g/L, which is a reasonable value for gases under atmospheric conditions.
Chemistry / Raymond Chang ,Williams College /(10th edition).
Fundamentals of Chemistry / David E.Goldberg/(5th edition).