A tank contains helium for filling balloons. It holds 8.00 L of He at 46.6 atm and 22.4 °C. What would be the volume of this helium at 2.14 atm and 14.0 °C?
PV = nRT
where:
P is the pressure of the gas = 46.6 atm
V is the volume of the gas = 8 Liter
n is the amount of substance of gas (in moles)
R is gas constant = = 0.0821 L atm K-1 Mol-1
T is the absolute temperature of the gas = 22.4 + 273 = 295.4 K
substitute in the equation and calculate Moles
n = 46.6 x 8 / 0.0821 x 295.4 = 15.37 moles
Using the mole value and above equation we can calcuate Volume of the baloon
P = 2.14 atm V = ?
n = 15.37 moles T = 273 +14 = 287
V = 0.0821 L atm K-1 Mol-1 x 15.37 moles x 287 K / 2.14 atm = 169.25 Liter
Hence Volume of the baloon is 169.25 Liter
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