Question

calculate molar mass of gas when density is 3.6kgm^-3
at 273 k and 1 atm​

Answer 1

Answer:

Given conditions ⇒

Density of the Carbon Dioxide = 1.965 kgm⁻³.

Temperature = 273 K.

Pressure = 1 atm.

Now, Using the Formula,

Pa/RT = Density

where, as is the molar mass of the gas

R is the gas constant equals to the 0.0821 liter-atm K⁻¹ mol⁻¹.

∴ 1 × a/(0.0821 × 273) = 1.965

∴ a = 1.965 × 0.0821 × 273

⇒ a = 44.04 ≈ 44 g/mol.

Hence, the molar mass of the Carbon Dioxide is approximately 44 g/mole.  

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Explanation:

Answer 2

Explanation:

Explanation:: The density of gas at 273 K and 1 atm pressure

=1.965kgm−3

=1.965kgm−3Molar mass of gas = don't know

At 273 K and 1 atm pressure, 1 mole of gas occupies a volume of 22.4 L

Mass of 1 mole of gas 3.6*0.083*273

Molar mass of gas= 81.57

So this is ur answer