Question

22.4 liters of CO2 at STP, 0◦C and 1 atm,

contains how many molecules? (Assume CO2
is an ideal gas.)

Answer 1

There are
`6.01* 10^(23)` number of molecules.

Step-by-step explanation:

Given that,

Volume, V = 22.4 L

Temperature, T = 0°C = 273.15 K

Pressure, P = 1 atm = 1.013 bar

We need to find the number of molecules. Let there are n number of molecules. We know that, ideal gas law is as follows :

`PV=nRT\\\\n=(PV)/(RT)\\\\n=(1.013* 22.4)/(0.08 314* 273.15)`

n = 0.999 moles

No. of molecules,

`N=n* N_A\\\\=0.999* 6.023* 10^(23)\\\\N=6.01* 10^(23)`

So, there are
`6.01* 10^(23)` number of molecules.