If 0.357 g of ch4 gas is introduced into an evacuated 1.75 l flask at 25°c, what is the pressure in
.08206 l atm/mol k)

P = 0.29 atm

Explanation:

Given data:

Mass of CH₄ = 0.357 g

Volume of flask = 1.75 L

Temperature = 25°C ( 25+273 = 298 K)

R = 0.08206 L. atm/K.mol

Pressure = ?

Solution:

Number of moles :

Number of moles = mass/ molar mass

Number of moles = 0.357 g /16g/mol

Number of moles = 0.02 mol

PV = nRT

P = nRT/V

P = 0.02 mol × 0.08206 L. atm/K.mol. × 298 K / 1.75 L

P = 0.5 L. atm  / 1.75 L

P = 0.29 atm

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