A steel tank with a volume of 2.924 L contains N2 gas under a pressure of 2.643 atm at 35.5 °C. Calculate?
6. A steel tank with a volume of 2.924 L contains N2 gas under a pressure of 2.643 atm at 35.5 °C. Calculate the number of moles of N2 in the tank.
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PV = nRT
P = pressure = 2.643 atm
V = volume = 2.924 L
n = moles = ? mol
R = gas constant = 0.082057 Latmmol^-1K^-1
T = temp in Kelvin = 35.5 deg C + 273.15 = 308.65 K
n = PV / RT
= 2.643 atm x 2.924 L / 0.082057 x 308.65 K
= 0.3051 mol
Use the appropriate gasoline equation PV=nRT P = a million.39 atm V = 75.0L T = 20 C = 293 ok R = .082 n = moles. for the reason that C2H2 has a molecular mass of 26 g / mol you could replace n with grams / mol mass. you've each of the counsel. Now in simple terms remedy for grams