A500 ml sample of a gas at 507 torr and 97 degrees celcius has a mass of 0.966g. what is the gas?

 the  gas  is identified  as follows

by  use  of  ideal  gas  equation  that is PV = nRT  where n  is  number  of  moles  calculate  the number of moles  involved

P=  507  torr
R(gass constant) = 62.364 L.torr/K.mol
T= 97 + 273 = 370 k
V  = 500ml = 500/1000= 0.5 Liters

by making n the  subject  of the  formula  n = PV/RT
= (507 torr x0.5 L)/ 62.364 L.torr/Mol.k   x  370  k) =  0.011  moles

the  molar  mass  of the  gas = mass/  number  of moles

= 0.966/0.011= 88 g/mol  =  the  gas is therefore  Krypton  since  88 g/mol is one of the isotope of  krypton