What is the molar mass and identity of a 5.28g sample of a gas that occupies 2.96 L at STP?

40 g/mol, Argon

Explanation:

We can find the number of moles of the gas by using the equation of state for an ideal gas:

where

is the pressure of the gas at STP

is the volume of the gas

n is the number of moles

is the gas constant

is the absolute temperature of the gas at STP

Solving for n, we find:

Now we can find the molar mass of the gas, which is given by

where

m = 5.28 g is the mass of the gas

n = 0.132 mol is the number of moles

Substituting,

So, the gas in this problem is Argon, which has a molar mass of 40 g/mol.

that's what i got you can count the number of atoms