At 300k and 1 bar density of gas is 2.5g/dm3.calculate it's molar mass.
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T= 300k,P=1bar,d=2.5g/dm^3,M=?
Wkt d=pm/Rt
=rtd/p=M
0.0821*2.5*300/1
=61.575 is the answer.
M=61.575
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T = 300 K
P = 1 bar = 1 atm = 1.013 * 10⁵ Pa
d = 2.5 gm/dm³ = 2.5 g/Liter = 2.5 kg/m³
The temperature and pressure are at STP. So one mole of the gas occupies 22.4 liters, assuming it as an ideal gas. Let there be n moles in the gas.
P V = n R T = m/M * R T
M = (m/V) * R T/P = d R T/P
= 2.5 kg/m³ * 8.314 J/K * 300 K / (1.103 * 10⁵ Pa )
= 0.0615 kg / mole
= 61.5 gm/mole
P = 1 bar = 1 atm = 1.013 * 10⁵ Pa
d = 2.5 gm/dm³ = 2.5 g/Liter = 2.5 kg/m³
The temperature and pressure are at STP. So one mole of the gas occupies 22.4 liters, assuming it as an ideal gas. Let there be n moles in the gas.
P V = n R T = m/M * R T
M = (m/V) * R T/P = d R T/P
= 2.5 kg/m³ * 8.314 J/K * 300 K / (1.103 * 10⁵ Pa )
= 0.0615 kg / mole
= 61.5 gm/mole
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