The volume of an ideal gas is 4.1 dm3 at 378.5 °C and 1 atm pressure
What is the volume (in liters) of the same amount of this gas at 304.4 °C and 1 atm pressure?
Universal Gas Constant = 8.314 J K−1 mol−1 = 0.082 L atm K−1mol−1
T(K) = T(°C) + 273.15
1.013 × 105 atm = 1 Pa = 1 N m-2
1000ml = 1l = 1 dm3
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Answer:
The ideal gas equation relating pressure (P), volume (V), and absolute temperature (T) is given as:
PV = nRT
Where,
R is the universal gas constant =8.314Jmol
−1
K
−1
n = Number of moles = 1
T = Standard temperature = 273 K
P = Standard pressure = 1 atm =1.013×10
5
Nm
−2
∴V=nRT/P
=1×8.314×273/(1.013×10
5
)
=0.0224m
3
=22.4 litres
Hence, the molar volume of a gas at STP is 22.4 litres.
Explanation:
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