A scuba diver is swimming 30m below the ocean surface where the pressure is 4 atm and the temperature is 8.0ᵒC. A bubble with a volume of 5mL is emitted from the breathing apparatus. What will the volume of the air bubble be when it is just below the surface of the water where the pressure is 101.3 kPa and the water temperature is 24.0ᵒC

A scuba diver is swimming 30m below the ocean surface where the pressure is 4 atm and the temperature is 8.0ᵒC. A bubble with a volume of 5mL is emitted from the breathing apparatus. What will the volume of the air bubble be when it is just below the surface of the water where the pressure is 101.3 kPa and the water temperature is 24.0ᵒC

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter5: The Gaseous State

Section: Chapter Questions

Problem 5.105QP: A glass tumbler containing 243 cm3 of air at 1.00 102 kPa (the barometric pressure) and 20C is...

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A scuba diver is swimming 30m below the ocean surface where the pressure is 4 atm and the temperature is 8.0C. A bubble with a volume of 5mL is emitted from the breathing apparatus. What will the volume of the air bubble be when it is just below the surface of the water where the pressure is 101.3 kPa and the water temperature is 24.0oC
The excess internal energy of metabolism is exhausted through a variety of channels, such as through radiation and evaporation of perspiration. Consider another pathway for energy loss: moisture in exhaled breath. Suppose you breathe out 25.0 breaths per minute, each with a volume of 0.630 L. Suppose also that you inhale dry air and exhale air at 36°C containing water vapor with a vapor pressure of 3.20 kPa. The vapor comes from the evaporation of liquid water in your body. Model the water vapor as an ideal gas. Assume its latent heat of evaporation at 36°C is the same as its heat of vaporization at 100°C. Calculate the rate at which you lose energy by exhaling humid air.
The pressure of the gas inside an aerosol can is 1.2 bar at a temperature of25 oC. Will the aerosol explode if it is thrown into a fire and heated to atemperature of 600 oC? Assume that the aerosol can is unable to withstandpressures in excess of 3 bar.
You and Liza Soberano are in an aircraft flying steadily at 4,300m above sea level and you are about to experience your first sky dive with her. You jumped first but Liza, due to hesitation, jumped after few seconds. Supposed that in an instant, the barometric pressure at your elevation is 85.0 kPa and Liza is higher from you by 800m. Determine the barometric pressure at Liza’s elevation assuming that pressure and temperature at sea level are 101.3 kPa and 25 deg.C respectively. Use lapse rate = 0.00650 K/m
The pressure of the gas inside an aerosol can is 1.2 bar at a temperature of25 C. Will the aerosol explode if it is thrown into a fire and heated to atemperature of 600 C? Assume that the aerosol can is unable to withstandpressures in excess of 3 bar.
Hot air balloons are often seen in early morning or right before the end of the day when it is cooler outside. This allows for the greatest difference in density between the hot air in the balloon and the outside air, and thus allows for the balloon to float more easily. If the outside air is 3 C, and the air inside of a hot air balloon is 50vC, calculate the densities of the air inside the balloon and outside the balloon. The air pressure is 102.0 kPa for both the balloon and the air. How many times more dense is the outside air than the air inside the balloon? Assume that the air in the balloon and in the air outside is made of nitrogen gas (N2).
Hot air balloons are often seen in early morning or right before the end of the day when it iscooler outside. This allows for the greatest difference in density between the hot air in the balloonand the outside air, and thus allows for the balloon to float more easily.If the outside air is 3oC, and the air inside of a hot air balloon is 50oC, calculate the densities ofthe air inside the balloon and outside the balloon. The air pressure is 102.0 kPa for both theballoon and the air. How many times more dense is the outside air than the air inside the balloon?Assume that the air in the balloon and in the air outside is made of nitrogen gas (N2). [
A researcher suspects that the pressure gauge on a 49.9 L gas cylinder containing nitric oxide is broken. An empty gas cylinder weighs 135 lb.The weight of the partially full cylinder is 149.6 lb.This cylinder is located in a relatively chilly service hallway at 287 K. Follow the steps below to use the compressibility charts to estimate the pressure of the gas and the reading that the pressure gauge should have. How many moles of nitric oxide, NO are in the cylinder? What is the ideal specific gravity for nitric oxide? What is the reduced temperature of the gas? What is the reduced pressure of the gas? What is the pressure inside the gas cylinder (absolute pressure)?
Determine the absolute pressure in torr on an object submerged 1000m below the surface of the sea. The density of sea water is 1020kg/m^3 and the acceleration due to gravity is 9.7 m/s^2. The local atmospheric pressure is 0.98 bar.
In the lungs, the respiratory membrane separates tiny sacs of air (absolute pressure=1.00x105 Pa) from the blood in the capillaries. These sacs are called alveoli, and it is from them that oxygen enters the blood. The average radius of the alveoli is 0.125 mm, and the air inside contains 14% oxygen, which is somewhat smaller amount than in fresh air. Assuming that the air behaves as an ideal gas at body temperature (310 K), find the number of oxygen molecules in one of the sacs.
An experiment is conducted in which a quantity of H2(g) is chemically generated in a closed headspace of volume V1 at absolute temperature T1, thereby raising the total pressure from Pa (the initial air pressure) to Pf (the total final pressure of H2(g) + air). Compose an algebraic expression for the volume (V2) that this sample of H2(g) would occupy if it were isolated (pure -- i.e. no air) at absolute temperature T2 and partial pressure P2. Note that your expression may contain no other variables than those given above, namely: V1, T1, T2, Pa, Pf, and P2. A) V2 = Now, suppose that the above experiment generated n mol of H2(g), that T2 = 0 °C and that P2 = 1 atm. Give the simple algebraic expression, in terms of V2 and n, which equates to the molar volume of H2(g) at STP. B) VM =
An experiment is conducted in which a quantity of H2(g) is chemically generated in a closed headspace of volume V1 at absolute temperature T1, thereby raising the total pressure from Pa (the initial air pressure) to Pf (the total final pressure of H2(g) + air).Compose an algebraic expression for the volume (V2) that this sample of H2(g) would occupy if it were isolated (pure -- i.e. no air) at absolute temperature T2 and partial pressure P2.Note that your expression may contain no other variables than those given above, namely: V1, T1, T2, Pa, Pf, and P2. V2 = Now, suppose that the above experiment generated n mol of H2(g), that T2 = 0 °C and that P2 = 1 atm. Give the simple algebraic expression, in terms of V2 and n, which equates to the molar volume of H2(g) at STP.VM = 8.829×10-4 mol of B2H6(g) (diborane gas) is generated into a 176.0 mL headspace, at 25.0 °C, thus increasing the pressure by 0.1209 atm. If we assume that the diborane gas obeys Boyle's Law and Charle's Law, what…

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