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- Calculate the steady state flux of nitrogen across a copper plate at 1200°C. The diffusion coefficient of N in Cu is D = 2.5 x 10- 11 m²/s, and the steady state concentration gradient is 0.4 kg/m³ across the 35 cm thick plate. Express your answer to one decimal place with the format x 10-11, in units of kg m-2 s-1How many moles of gas are pressured in a 6,000,000 mcL chamber containing a pressure of 960 mmHg at – 25 deg C?The air quality index in Beijing last year recorded average ozone (O3) levels of 110 ppb (on a mol basis). Does this exceed Canada's acceptable 24 hour National Ambient Air Quality Objective (NAAQO) of 50 micrograms/M3? Assume the average molar mass of air is 29.0 g/mol and its density is 1.225 kg/M3.
- Compute the density in units of of an ideal gas under the following conditions: a) At and Torr pressure (1 Torr = 1mm Hg) this is called loschmidt number. b) In a vacuum of Torr at room temperature . This number is useful one for the experimentalist to know by heart. (10^-3 Torr = 1 micron)Using the ideal gas law, PV = nRT, determine the volume 200 lbs of hydrogen would occupy at 180 degrees F and a pressure of 100 psig? Assume the constant “R” is 10.731 Ft3PSIA/0R lb mole and the molecular weight of H2 is 2 lbs./mole.Find the K.E. (1) per cm³ (2) per mole (3) per gram and (4) per molecule of nitrogen at N.T.P. (Molecular weight of N₂ 28, Normal pressure = 76 cm of mercury, density of Hg 13.6 gm/cm³ g = 980 cm/s², Avogadro's number 6.023 x 1023 molecules/mole. (R = 8.314 x 10² erg/mole K)
- The rate of change of atmospheric pressure P with respect to altitude h is proportional to P, provided that the temperature is constant. At 15°C the pressure is 101.3 kPa at sca level and 87.14 kPa at h = 1000 m. (a) What is the pressure at an altitude of 3000 m? (b) What is the pressure on top of Mount McKinley, at an altitude of 6187 m?Pls help on this question.For divers going to great depths, the composition of the air in the tank must be modified. The ideal composition is to have approximately the same number of O2 molecules per unit volume as in surface air (to avoid oxygen poisoning), and to use helium instead of nitrogen for the remainder of the gas (to avoid nitrogen narcosis, which results from nitrogen dissolving in the bloodstream). Of the molecules in dry surface air, 78.0% are N2, 21.0% are O2, and 1.00% are Ar. (Assume that the density of seawater is 1025 kg/m3 and the temperature is 20.0°C.) Density of dry air at 20.0°C is 1.20 kg/m3. Molar mass of N2 is 14.007 g/mol, O2 is 15.999 g/mol, and Ar is 39.948 g/mol. For a diver going to a depth of 141 m, what percentage of the gas molecules in the tank should be O2?
- Presents the diagram of the problem, necessary formulas, clearance and numerical solution: On June 26, the US Brookhaven National Laboratory (BNL) announced that the Guinness World Records (GWR) organization had granted him the temperature record highest ever achieved: gold ion collisions at nearly the speed of light at the accelerator of Relativistic Heavy Ion Collider particles had formed a plasma at 4 billion degrees Celsius. Convert this value to ◦C and K.HAND WRITTEN Plz..I'll upvote For a mixture of 40% nitrogen, 35% oxygen, and 25% carbon dioxide on a molar basis, what is the mixture constant a in the equation P=R ? Express your answer in kPa(m³/kmol)2K1/2 (+4)7If the dew point of air (35°C and 1 atm) is 20 °C, what is the RH under that temperature and pressure (35°C and 1 atm)? What is the volume fraction?
