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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-1The 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.What is the bulk density of the dry soil?
- 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.The escape velocity of any object from Earth is 11.2 km/s. (a) Express this speed in m/s and km/h. Speed, m/s: 11200 Speed, km/h: 40320 (b) At what temperature would oxygen molecules (molecular mass is equal to 32 g/mol) have an average velocity, v, 'ms' equal to Earth's escape velocity 11.2 km/s? Temperature: 1,89 ×108 K No, that's only partially correctFind 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)
- Pls help on this question.Try to answer in 30 minuteA) What is an equation to equate KE and GPE? B) A gas is held in a container of 15 m^3 in volume and a pressure of 5 Pa. If the volume isincreased to 26 m^3 what is the pressure of the gas? c)A syringe has a volume of 5 cm^3 and a temperature of 300 k. Upon heating the syringeexpands to a volume is now 5.5cm^3, what is the temperature of the syringe?
- 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?A cylinder contains 0.020 m3 of molecular oxygen at a temperature of 25 C and a pressure of 15 atm. What would be the volume of this gas at a pressure of an atmosphere? A patient breathes this oxygene using a mask has a rate 0.0080 m3/minute at atmospheric pressure. After how long will the cylinder be 'empty' i.e. its pressure will be 1 atm.If 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?
