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- Which postulate of the kinetic molecular theory breaks down under conditions of low temperature?
Problem 1
- Suppose that the exhaust stream of an automobile has a flow rate of 2.55 L/s at 655 K and contains a partial pressure of NO of 12.4 torr. What total mass of urea is necessary to react completely with the NO formed during 8.0 hours of driving?
Problem 11
Problem 25a
The pressure in Denver, Colorado (elevation 5280 ft), averages about 24.9 in Hg. Convert this pressure to each indicated unit. a. atm
Problem 25b
The pressure in Denver, Colorado (elevation 5280 ft), averages about 24.9 in Hg. Convert this pressure to each indicated unit. b. mmHg
Problem 25c
The pressure in Denver, Colorado (elevation 5280 ft), averages about 24.9 in Hg. Convert this pressure to each indicated unit. c. psi
Problem 25d
The pressure in Denver, Colorado (elevation 5280 ft), averages about 24.9 in Hg. Convert this pressure to each indicated unit. d. Pa
Problem 26
The pressure on top of Mount Everest (29,029 ft) averages about 235 mmHg. Convert this pressure to each indicated unit. a. torr b. psi c. in Hg d. atm
Problem 27a
The North American record for highest recorded barometric pressure is 31.85 in Hg, set in 1989 in Northway, Alaska. Convert this pressure to each indicated unit. a. mmHg
Problem 28b
The world record for lowest pressure (at sea level) was 652.5 mmHg recorded inside Typhoon Tip on October 12, 1979, in the western Pacific Ocean. Convert this pressure to each indicated unit. b. atm
Problem 28d
The world record for lowest pressure (at sea level) was 652.5 mmHg recorded inside Typhoon Tip on October 12, 1979, in the western Pacific Ocean. Convert this pressure to each indicated unit. d. psi
Problem 32a
Given a barometric pressure of 751.5 mmHg, calculate the pressure of each gas sample as indicated by the manometer.
(a)
Problem 32b
Given a barometric pressure of 751.5 mmHg, calculate the pressure of each gas sample as indicated by the manometer.
(b)
Problem 33
A sample of gas has an initial volume of 4.20 L at a pressure of 755 mmHg. If the volume of the gas is increased to 7.10 L (at constant temperature), what is its pressure?
Problem 34
A sample of gas has an initial volume of 14.1 L at a pressure of 1.05 atm. If the sample is compressed to a volume of 10.1 L (at constant temperature), what is its pressure?
Problem 35
A 48.3-mL sample of gas in a cylinder is warmed from 22 °C to 87 °C. What is its volume at the final temperature?
Problem 36
A syringe containing 1.55 mL of oxygen gas is cooled from 95.3 °C to 0.0 °C. What is the final volume of oxygen gas?
Problem 37
A balloon contains 0.119 mol of gas and has a volume of 3.21 L. If an additional 0.103 mol of gas is added to the balloon (at constant temperature and pressure), what is its final volume?
Problem 38
A cylinder with a moveable piston contains 0.221 mol of gas and has a volume of 178 mL. What is its volume if an additional 0.244 mol of gas is added to the cylinder? (Assume constant temperature and pressure.)
Problem 41a
What volume is occupied by 0.118 mol of helium gas at a pressure of 0.97 atm and a temperature of 305 K?
Problem 41b
What volume is occupied by 0.118 mol of helium gas at a pressure of 0.97 atm and a temperature of 305 K? Would the volume be different if the gas was argon (under the same conditions)?
Problem 42
What volume is occupied by 12.5 g of argon gas at a pressure of 1.05 atm and a temperature of 322 K? Would the volume be different if the sample were 12.5 g of helium (under identical conditions)?
Problem 44
What is the pressure in a 19.0-L cylinder filled with 34.3 g of oxygen gas at a temperature of 312 K?
Problem 46
What is the temperature of 3.05 g of helium gas at a pressure of 1.70 atm and a volume of 14.1 L?
Problem 49
An automobile tire has a maximum rating of 38.0 psi (gauge pressure). The tire is inflated (while cold) to a volume of 11.8 L and a gauge pressure of 36.0 psi at a temperature of 12.0 °C. On a hot day, the tire warms to 65.0 °C, and its volume expands to 12.2 L. Does the pressure in the tire exceed its maximum rating? (Note: The gauge pressure is the difference between the total pressure and atmospheric pressure. In this case, assume that atmospheric pressure is 14.7 psi.)