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- A plastic bag is weighed and then filled successively with two gases, X and Y. The following data are gathered: Temperature: 0.0°C (273 K) Pressure: 1.00 atmosphere Mass of empty bag: 20.77 g Mass of bag filled with gas X: 24.97 g Mass of 1.12 liters of air at conditions given: 1.30 g Volume of bag: 1.12 liter Molar volume at STP: 22.4 liters Reference: Ref 5-6 The bag is emptied and refilled, successively, with gases X and Y, this time at 1 atm pressure and a temperature 30°C higher. Assume that the volume of the bag is the same as before. Which one of the following statements is wrong? Select one: a. The full bag contains fewer molecules of each gas than it did at 0.0°C. b. The ratio of the density of gas Y to the density of gas X is the same as at 0.0°C. c. The molar masses of the two gases are the same as they were at 0.0°C. d. The mass of each gas filling the bag is now 303/273 times…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…
- 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 plastic bag is weighed and then filled successively with two gases, X and Y. The following data are gathered: Temperature: 0.0°C (273 K) Pressure: 1.00 atmosphere Mass of empty bag: 20.77 g Mass of bag filled with gas X: 24.97 g Mass of 1.12 liters of air at conditions given: 1.30 g Volume of bag: 1.12 liter Molar volume at STP: 22.4 liters Reference: Ref 5-6 The mass of 1.12 liters of gas Y is found to be 6.23 g. The density of gas Y is Select one: a. 10.6 g/L b. 5.56 g/L c. 15.6 g/L d. 0.200 g/L e. 0.180 g/LGypsum (plaster of Paris : CaSO,. 2H,0) is produced by the reaction of calcium carbonate and sulfuric acid. A certain lime stone analyzes: CaCO, 96.89 %; MgCO, 1.41 %; inerts 1.70 %. For 5 metric tons of limestone reacted completely, determine: a. kg of anhydrous gypsum (CaSO,) produced. b. kg of sulfuric acid solution (98 wt%) required.
- The molar mass of a newly synthesized fluorocarbon was measured in a gas microbalance. This device consists of a glass bulb forming one end of a beam, the whole surrounded by a closed container. The beam is pivoted, and the balance point is attained by raising the pressure of gas in the container, so increasing the buoyancy of the enclosed bulb. In one experiment, the balance point was reached when the fluorocarbon pressure was 327.10 Torr; for the same setting of the pivot, a balance was reached when CHF3 (M = 70.014 g mol−1) was introduced at 423.22 Torr. A repeat of the experiment with a different setting of the pivot required a pressure of 293.22 Torr of the fluorocarbon and 427.22 Torr of the CHF3. What is the molar mass of the fluorocarbon? Suggest a molecular formula.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 =At a certain location the surface temperature is 34⁰C and the lapse rate is -8.7⁰C/1,000 m. A parcel of air with a temperature of 28⁰C has been lifted to an altitude of 950 m. Is the parcel of air stable or unstable?
- Derive an expression that shows how the pressure of a gas inside an effusion oven (a heated chamber with a small hole in one wall) varies with time if the oven is not replenished as the gas escapes. Then show that t1/2, the time required for the pressure to decrease to half its initial value, is independent of the initial pressure. Hint: Start from the expression for the rate of effusion and rewrite it as a differential equation relating dp/dt to p; recall that pV = NkT can be used to relate the pressure to the number density.A tanker truck carrying liquid ammonia overturns, releasing ammonia vapor into the air.(a) Approximating ammonia, oxygen, and nitrogen asspheres of equal diameter (3 × 10-10 m), estimate the diffusion constant of ammonia in air at atmosphericpressure and 20°C.(b) Calculate the time required for a 100-m root-meansquare displacement of ammonia from the truck, andexpress this time in everyday units (seconds, minutes,hours, days, or years). The actual time for the ammonia to travel this distance is far shorter because of theexistence of air currents (even when there is no wind).Ammonia gas (A) diffuses through a stagnant gas mixture consisting of one-third Nitrogen (B) and two thirds Hydrogen (C) by volume. The total pressure is 206.8 kN/m2 and the temperature is 540c.Calculate the rate of diffusion of Ammonia through a film of gas 0.5mm thick when the concentration change across the film is 10% to 5% by volume. The diffusivities at 200 0 c and one std. atm.pressure are reported to be DAB = 5.391 x 10 -4 m2 /s and DAC = 1.7371 x 10 -4 m2 /s.