Respuesta :
Explanation:
The given data is as follows.
   Volume = 5.8 L,   Pressure = 1.00 atm
   T = [tex]21^{o}C[/tex] = (21 + 273) K = 294 K,  mass = 6.7 g
   R = 0.0821 Latm/mol K
According to the ideal gas equation, we will calculate the number of moles as follows.
       PV = nRT
or, Â Â Â Â Â n = [tex]\frac{PV}{RT}[/tex]
Hence, putting the given values into the above formula as follows.
        n = [tex]\frac{PV}{RT}[/tex]
         = [tex]\frac{1.00 atm \times 5.8 L}{0.0821 Latm/mol K \times 294 K}[/tex]
         = 0.24 mol
Now, calculate molar mass of the gas as follows.
      Molar mass = [tex]\frac{mass}{\text{no. of moles}}[/tex]
                = [tex]\frac{6.7 g}{0.24 mol}[/tex]
                = 27.91 g/mol
or, Â Â Â Â Â Â Â Â Â Â Â Â Â Â = 28 g/mol (approx)
As the gas is diatomic so, mass of two atoms of gas X is 28 g/mol. And, mass of one atom of gas is as follows.
           [tex]\frac{28 g/mol}{2}[/tex]
             = 14 g/mol
Hence, nitrogen atom has a mass of 14 g/mol. Therefore, we can conclude that the given diatomic gas is [tex]N_{2}[/tex].
