how many grams of H2 gas are present in a 44.0 L fuel tank at a pressure of 2720 lb/in2 (psi) at 20 degrees Celsius? Assume that 1 atm= 14.7 psi.
Volume = 44.0L
Pressure = 2720 lb/in2 =2720/14.7 atm =185.03atm
T = 20oC = 293K
Apply ideal gas equation to find no. of moles of H2 present in tank.
PV = nRT
P = pressure in tank =185.03atm
V = volume of tank = 44.0L
n = no. of moles of gas present.
R = real gas constant = 0.082 L atm K-1 mol-1
T = temperature of tank = 293K
185.03*44.0 = n*0.082*293
n = 338.854
No. of moles of H2 present in tank is 338.854.
moles = given mass/mass of given compound
338.854 = given mass/2
given mass = 677.708g
So 677.708g of H2 gas is present in the tank.
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