Answered: 8. What is the molar fraction of air…

8. What is the molar fraction of air component? Evaluate the average density of air at T = 25 °C. also evaluate the molecular weight of air at the same temperature?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter5: Gases

Section: Chapter Questions

Problem 28QAP: Exhaled air contains 74.5% N2, 15.7% O2, 3.6% CO2, and 6.2% H2O (mole percent). (a) Calculate the...

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The gas in the discharge cell of a laser contains (in mole percent) 11% CO2, 5.3% N2, and 84% He. (a) What is the molar mass of this mixture? (b) Calculate the density of this gas mixture at 32C and 758 mm Hg. (c) What is the ratio of the density of this gas to that of air (MM=29.0g/mol)at the same conditions?
Exhaled air contains 74.5% N2, 15.7% O2, 3.6% CO2, and 6.2% H2O (mole percent). (a) Calculate the molar mass of exhaled air. (b) Calculate the density of exhaled air at 37C and 757 mm Hg and compare the value you obtained with that of ordinary air (MM=29.0g/mol) under the same conditions.
At the critical point for carbon dioxide, the substance is very far from being an ideal gas. Prove this statement by calculating the density of an ideal gas in g/cm3 at the conditions of the critical point and comparing it with the experimental value. Compute the experimental value from the fact that a mole of CO2 at its critical point occupies 94 cm3.
A flask containing 161 cm ^ 3 of hydrogen was collected under a pressure of 29.5 kPa. What pressure would have been required for the vol ume of the gas to have been 80 cm ^ 3 , assuming the same temperature ? Answer in units of kPa .
1. The lung capacity of a scuba diver at the surface of the water is 3200 mL at 17°C and standard pressure. The diver goes to a depth where the pressure is 202 kPa and the temperature is 7°C. Calculate the volume of air that his lungs could hold at that depth.
The effect of high pressure on organisms, including humans, is studied to gain information about deep-sea diving and anaesthesia. A sample of air occupies 1.00 dm3 at 25°c and 1.00 atm. What pressure is needed to compress it to 100 cm3 at this temperature?
What would be the height of the column in a barometerif the external pressure was 101 kPa and water1d = 1.00 g>cm32 was used in place of mercury?(a) 0.0558 m (b) 0.760 m (c) 1.03 * 104 m(d) 10.3 m (e) 0.103 m
What is the mass of air contained in a room 6 m × 10 m × 4 m if the pressure is 100 kPa andthe temperature is 25°C?
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. V2 = VM =
What would be the height of the column in a barometerif the external pressure was 101 kPa and water(d = 1.00 g/cm3) was used in place of mercury?(a) 0.0558 m (b) 0.760 m (c) 1.03 x 104 m(d) 10.3 m (e) 0.103 m
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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