Question

Calculate the density of CO2 in g/cm3 at room temperature(25 degrees Celsuis) and pressure(1 atm) assuming it acts as an ideal gas

Answer 1

`density=1.8x10^(-3)g/mL`

Step-by-step explanation:

Hello,

Considering the ideal equation of state:

`PV=nRT`

The moles are defined in terms of mass as follows:

`n=(m)/(M)`

Whereas
`M` the gas' molar mass, thus:

`PV=(mRT)/(M)`

Now, since the density is defined as the quotient between the mass and the volume, we get:

`P=(m)/(V) (RT)/(M)`

Solving for
`m/V`:

`density= m/V=(PM)/(RT)`

Thus, the result is given by:

`density=((1atm)(44g/mol))/([0.082atm*L/(mol*K)]*298.15K) \\density=1.8g/L=1.8x10^(-3)g/mL`

Best regards.