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

Answer:

There are $6.01\times 10^{23}$ number of molecules.

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 :

$PV=nRT\\\\n=\dfrac{PV}{RT}\\\\n=\dfrac{1.013\times 22.4}{0.08 314\times 273.15}$

n = 0.999 moles

No. of molecules,

$N=n\times N_A\\\\=0.999\times 6.023\times 10^{23}\\\\N=6.01\times 10^{23}$

So, there are $6.01\times 10^{23}$ number of molecules.