The molecular weight of 2.6g of a gas which occupies 2.24 litres at 0 degrees Celsius and 760 mm pressure
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If the gas is ideal then
P = 760 mm of Hg = 1 atm
T = 0°C = 273 K
R = 0.0821 atm L / (mol K)
n = PV / (RT)
= (1 atm × 2.24 L) / (0.0821 atm L / (mol K) × 273 K)
= 0.1 moles
Molecular weight = Weight / No. of moles
= 2.6 g / 0.1 mol
= 26 g / mol
Molecular weight of given gas is 26 g/mol
P = 760 mm of Hg = 1 atm
T = 0°C = 273 K
R = 0.0821 atm L / (mol K)
n = PV / (RT)
= (1 atm × 2.24 L) / (0.0821 atm L / (mol K) × 273 K)
= 0.1 moles
Molecular weight = Weight / No. of moles
= 2.6 g / 0.1 mol
= 26 g / mol
Molecular weight of given gas is 26 g/mol
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