Question 3. At 100°C and 16.0 kPa, the mass density of phosphorus vapour is0.6388 kg m-3. What is the molecular formula of phosphorus under theseconditions?
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Question 3. At 100°C and 16.0 kPa, the mass density of phosphorus vapour is
0.6388 kg m-3. What is the molecular formula of phosphorus under these
conditions?
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Solved in 2 steps
- (a) A rigid tank contains 1.60 moles of helium, which can be treated as an ideal gas, at a pressure of 28.0 atm. While the tank and gas maintain a constant volume and temperature, a number of moles are removed from the tank, reducing the pressure to 5.00 atm. How many moles are removed? mol (b) What If? In a separate experiment beginning from the same initial conditions, including a temperature T, of 25.0°C, half the number of moles found in part (a) are withdrawn while the temperature is allowed to vary and the pressure undergoes the same change from 28.0 atm to 5.00 atm. What is the final temperature (in °C) of the gas? °CA mixture of CO2 and Kr weighs 37.6 g and exerts a pressure of 0.855 atm in its container. Since Kr is expensive, you wish to recover it from the mixture. After the CO2 is completely removed by absorption with NaOH(s), the pressure in the container is 0.293 atm. (a) How many grams of CO2 were originally present? (b) How many grams of Kr can you recover? (a) grams CO2: (b) grams Kr: 3. 8.A mixture of CO₂ and Kr weighs 29.6 g and exerts a pressure of 0.895 atm in its container. Since Kr is expensive, you wish to recover it from the mixture. After the CO₂ is completely removed by absorption with NaOH(s), the pressure in the container is 0.295 atm. (a) How many grams of CO₂ were originally present? (b) How many grams of Kr can you recover? (a) grams CO₂: g (b) grams Kr:
- 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 328C and 758 mm Hg. (c) What is the ratio of the density of this gas to that of air (MM air = 29.0 g/mol) at the same conditions5.(a) Assume for the moment that air consist of 80.00% nitrogen and 20.00% oxygen byvolume. Use these figures and typical values for temperature and pressure (1.000atm, 25.0 ºC) to calculate the density of air. (b) This calculation affords a good approximation of the density of air at sea level.However, your lab is at an altitude approximately 777 meters (2550 feet). Knowingthis, will the density of air in you lab be higher or lower than the value you justcalculated? Why? (c) Besides altitude, what else affects the atmospheric pressure? Where could you findthe actual atmospheric pressure at the time of the experiment?The size of the ionic atmosphere, called the Debye radius, is 1/K, where K is given by e2 NA 1/2 VI E0 ɛkBT K = where e is the electronic charge, NA Avogadro's constant, ɛo the permittivity of vacuum (8.854×10-12 c²·n-1.m-2), ɛ the dielectric constant of the solvent, kB the Boltzmann constant, T the absolute temperature, and I the ionic strength. Calculate the Debye radius in a 0.036 m aqueous Na2S203 solution at 25°C. (Assume the density of the solution at 25°C is 1.0029 g•cm-3.) 4.0 4.208 Å
- (a) The molecular diameter of helium, He, is 0.225 nm. At 0 °C and 101.325 kPa, calculate the (iv) mean free path, A. (v) collision frequency, ZA. (vi) collision density, Za. 2.If 400cm^3 of Q was collected at 25°c and 1.20 x10^5, calculate the volume it would occupy at s.t.p and the number of molecules of Q present.(standard pressure=1.0 x 10^5 Nm^-2 Avogadro's constant= 6.023 x 10^23, 1 mole of gas occupies 22.4 dm^3 at s.t.p)1. At an altitude of 150 km, the pressure is about 2.7 x 10-⁹ bar and T≈ 500 K. (a) Assuming for simplicity that the air consists entirely of nitrogen, calculate the mean free path (in m) under these conditions. For N₂ molecules o=4.50 × 10-19 m². (b) What is the average collision frequency (in sec-¹) between N₂ molecules?
- 4. Atmospheric compositionUse the following data from the U.S. Standard Atmosphere Model to calculate themolar mass at each point in the atmosphere.Sea Level T = 288.2 K, p = 101, 325 Pa, ρ = 1.225 kg/m3LEO (400 km) T = 995.8 K, p = 1.45 × 10−6 Pa, ρ = 2.8 × 10−12 kg/m3The mass density of a gaseous compound was found to be 1.23 kg m−3 at 330 K and 20 kPa. What is the molar mass of the compound?The size of the ionic atmosphere, called the Debye radius, is 1/K, where k is given by e? NA" 1/2 Vi K = where e is the electronic charge, NA Avogadro's constant, ɛo the permittivity of vacuum (8.854×10-12 c2.N-1.m-2), ɛ the dielectric constant of the solvent, kg the Boltzmann constant, T the absolute temperature, and I the ionic strength. Calculate the Debye radius in a 0.036 m aqueous Na2S203 solution at 25°C. (Assume the density of the solution at 25°C is 1.0029 g•cm¬3.) 4.0 Å
