A 500 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