Question

A certain gas occupies 0.15m^3 at 20°c and 1.2 bar. if gas has mass of 200g. Calculate:
a) value of gas constant
b) molecular mass of the gass​

Answer 1

Answer:

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Explanation:

Answer 2

Answer:

a) The value of the gas constant is $0.0831\hspace{1mm} L.bar.K^{-1} mol^{-1}$. b) The molecular mass of the gas is $27.067\hspace{1mm} g/mol$.

Explanation:

• The temperature, volume, and pressure of a gas are related, by the ideal gas law.
• At a constant temperature, Boyle's law is applicable.

The formula for the ideal gas law is:

$PV=nRT$

where $P$ is the pressure of the gas

           $V$ is the volume.

           $n$ is the number of moles of the gas.

           $R$ is the gas constant

           $T$ is the temperature.

Solution Part a):

The gas constant $(R)$ is a universal constant. The value of the gas constant is $0.0831\hspace{1mm} L.bar.K^{-1} mol^{-1}$.

Solution Part b):

It is given that:

$P=1.2\hspace{1mm} bar$

$V= 0.15\hspace{1mm} m^{3}$

   $=150\hspace{1mm} L$

$T=(20 + 273.15)\textdegree K$

  $=293.15$ $\textdegree K$

$PV=nRT$

$(1.2\hspace{1mm} bar)\times(150 \hspace{1mm} L)=(\frac{200\hspace{1mm} g}{M} ) \times (0.0831\hspace{1mm} L.bar.K^{-1} mol^{-1})\times (293.15\textdegree K)$

$M= (\frac{200\times 0.0831\times 293.15}{1.2\times 150} )\hspace{1mm} g/mol$

$M=27.067\hspace{1mm} g/mol$

So, the molecular mass of the gas is $27.067\hspace{1mm} g/mol$.