What is the likely identity of a gas at #273.15# #K#, whose mass is #7.5*g#, and which exerts a pressure of #1*"bar"#?

1 Answer
Jun 19, 2017

Answer:

Well, let's try to address the molar mass of the gas........we get a range of possibilities.........

Explanation:

#"STP"# specifies a temperature of #273.15 K#, and an absolute pressure of exactly #100* kPa, "1 bar"#.

#n=(PV)/(RT)=(1*cancel"bar"xx5.6*cancelL)/(8.314xx10^(-2)cancelL*cancel"bar"*cancel(K^-1)*mol^-1xx273.15*cancelK)#

#=0.247*(mol^-1)^-1=0.247*mol#

And thus #(7.5*g)/(0.247*mol)=30.3*g*mol^-1#.

The gas is likely the homonuclear diatomic #N_2# or #O_2#.

Further data are needed to confirm the identity of the gas.