The velocity of air in a 0.08 m² air duct is 5 m/s. How much air can pass through the duct in a winter day at -20 °C? Assume atmospheric pressure as 1 atm (MW Air= 28.9 g/mol, R = 0.08205 liter.atm/mol.K) and air behaves as an ideal gas. 415244 kg/day 480856 kg/day 41524.4 kg/day

The velocity of air in a 0.08 m² air duct is 5 m/s. How much air can pass through the duct in a winter day at -20 °C? Assume atmospheric pressure as 1 atm (MW Air= 28.9 g/mol, R = 0.08205 liter.atm/mol.K) and air behaves as an ideal gas. 415244 kg/day 480856 kg/day 41524.4 kg/day

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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One type of gas mixture used in anesthesiologyis a 50%/50% mixture (by volume) of nitrous oxide (N2O) and oxygen(O2), which can be premixed and kept in a cylinder for later use.Because these two gases don’t react chemically at or below 2000 psi, attypical room temperatures they form a homogeneous single gas phase,which can be considered an ideal gas. If the temperature drops below-6C, however, N2O may begin to condense out of the gas phase. Thenany gas removed from the cylinder will initially be nearly pure O2; asthe cylinder empties, the proportion of O2 will decrease until the gascoming from the cylinder is nearly pure N2O. In another test, the valve of a 500 L cylinder full of the gas mixture at 2000 psi (gauge pressure) is opened wide so that the gas rushes out of the cylinder very rapidly. Why might some N2O condense during this process? (a) This is an isochoric process in which the pressure decreases, so the temperature also decreases. (b) Because of the rapid expansion, heat is…
A compressed gas cylinder at 13,700 kPa and 23°C, is in a room where a fire raises the temperature to 450.°C. What is the new pressure of the cylinder, in atm? The volume of the cylinder does not change.
Everything needed is included. An empty 1.0-liter cylinder is filled with 48.0 grams of methane (CH4 ) at 273 K. 2a. Predict (calculate) the pressure, assuming methane behaves as an ideal gas. 2b. Suppose the pressure is measured and is found to actually be 56 atm. Determine the compression factor Z, and indicate whether attractive or replusive intermolecular forces are dominant in methane under these conditions.
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At a constant temperature, an ideal gas is compressed from 6.0 Liters to 4.0 Liters by a constant external pressure of 5.00 atm. 1 atm =1.01 x 10° Pa Answer the following questions by filling in the blanks a. What is the constant external pressure applied to the gas in Pa? Represent your answer with 3 significant figure using scientific notation, without units.e.g. 1.23E+3 The external presure applied to the gas is Pa b. What is the change in volume of the gas in Liters? Represent your answer with 1 decimal place using normal notation, without units. The change in volume of the gas is C. What is the change in volume of the gas in m3? Represent your answer with 3 significant figure using normal notation, without units. The change in volume of the gas is m3 d. How much work (in kJ) is done on the gas? Represent your answer with 3 decimal.places using normal.notation, without units The work done on the gas is kJ 16°C Sunny
Two flasks of equal volume are connected by a narrow tube (of negligible volume). Initially, both flasks are at 27°C and contain 0.70 moles of hydrogen gas, the pressure being 50,000 Pa. One of the flasks is then immersed in a hot oil bath at 127°C, while the other is kept at 27°C. Calculate the final pressure of the system, in Pa. Calculate the final number of moles of hydrogen gas in the flask that was immersed in the oil bath. R = 0.08205 L atm mol-¹ K-₁ T(K) = T (°C) + 273.15