At an altitude of 11,000 m (a typical cruising altitude for a jet airliner), the air temperature is -60.0 ∘C and the air density is 0.491 kg/m3. The molar mass of air is 28.8 g/mol. What is the pressure of the atmosphere at that altitude? (Note: The temperature at this altitude is not the same as at the surface of the earth, so the equation P=P0exp(−MgyRT) doesn't apply.)

A bicycle tire contains 2.00 L of gas at an absolute pressure of 7.00 × 105 N/m2 and a temperature of 18.0 °C . What will its pressure be if you let out an amount of air that has a volume of 100 cm3 at atmospheric pressure? Assume tire temperature and volume remain constant.

A helium filled weather balloon has a volume of 3.0 m3 at lift off where the air pressure is 1 atm and the temperature is 20oC.  When airborne the temperature is -60oC and its volume expands to 120 m3.  What is the pressure at the airborne location? 0.0058 atm 0.0083 atm 0.018 atm 0.034 atm

A bag of potato chips contains 2.00 L of air when it is sealed at sea level at a pressure of 1.00 atm and a temperature of 20.0°C. What will be the volume of the air in the bag if you take it with you, still sealed, to the mountains where the temperature is 7.00°C and atmospheric pressure is 70.0 kPa? Assume that the bag behaves like a balloon and that the air in the bag is in thermal equilibrium with the outside air. (1 atm = 1.01 × 105 Pa)

A bag of potato chips contains 2.00 L of air when it is sealed at sea level at a pressure of 1.00 atm and a temperature of 20.0°C. What will be the volume of the air in the bag if you take it with you, still sealed, to the mountains where the temperature is 7.00°C and atmospheric pressure is 70.0 kPa? Assume that the bag behaves like a balloon and that the air in the bag is in thermal equilibrium with the outside air. (1 atm = 1.01 × 105 Pa)   a. 4.13 L    b. 1.01 L     c. 1.38 L     d. 2.76 L

The density of air at 20 degree celcius is 1.204 kg/m3. The density at temperature 100 degree celcius is 0.9467 kg/m3. If an average size hot air balloon envelopes a volume of 2200 m3, how much weight can it lift (including the balloon itself)? a. 5.55 kN b. 11.1 kN c. 20.4 kN d. 26.0 kN

A bicycle tire has a pressure of 6.95 × 105 Pa at a temperature of 16°C and contains 2.00 L of gas. a)What will its pressure be, in pascals, if you let out an amount of air that has a volume of 105 cm3 at atmospheric pressure and at the temperature of the tire? Assume tire temperature and volume remain constant.

Suppose you have a large hot air balloon, open at the bottom but filled with air that is heated to 50 °C while the outside air is 10 °C.  What can you say about the air inside the balloon and how much it can lift?   The density of air is surprisingly high: 1.23 kg/m3, an average hot air balloon has a volume of 3000 m3 , and the acceleration of gravity is 9.8 m/s2.     The density is  higher by the factor (273 + 50)/(273+10) = 1.14 and therefore will not have a buoyant force and will not lift off the ground with any load.       The density is lower by the factor (273 + 10)/(273+50) = 0.88 and therefore will have a buoyant force of 0.88 times the weight of the air it replaced, or about 32,000 N.        The density is lower by the factor (273 + 10)/(273+50) = 0.88 and therefore will have a buoyant force of 0.12 times the weight of the air it replaced, or about 4300 N.        The density is the same but the pressure of the hot air is higher by (273 + 50)/(273+10) =…

In one observation, the column in a mercury barometer has a measured height h of 740.35 mm.The temperature is 5.0 C, at which temperature the density of mercury r is 1.3608 * 10^4 kg/m3.The free-fall acceleration g at the site of the barom- eter is 9.7835 m/s2.What is the atmospheric pressure at that site in pascals and in torr (which is the common unit for barometer readings)?

A deep sea diver should breathe a gas mixture that has the same oxygen partial pressure as at sea level, where dry air contains 20.9% oxygen and has a total pressure of 1.01 ✕ 105 N/m2. (a) What is the partial pressure (in N/m2) of oxygen at sea level? N/m2 (b) If the diver breathes a gas mixture at a pressure of 2.00 ✕ 106 N/m2, what percent oxygen should it be to have the same oxygen partial pressure as at sea level? %