1L of NH3 2L of Cl2 8L of He 4L of CO2

At STP 4 liters of O2 contains the same total number of molecules as

See your post above.

2L of Cl2

To compare the number of molecules in different gases at standard temperature and pressure (STP), we can use the Ideal Gas Law. The Ideal Gas Law equation is written as PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

At STP, the temperature is 273.15 Kelvin, and the pressure is 1 atmosphere.

First, we need to calculate the number of moles in each gas using the given volume and the molar volume of a gas at STP, which is 22.4 L/mol.

For O2 (oxygen gas), we have 4 liters. So the number of moles (n) of O2 can be calculated as:

n(O2) = V(O2) / V(molar_O2)
= 4 L / 22.4 L/mol
= 0.179 moles

Now we can calculate the number of molecules in 0.179 moles of O2 using Avogadro's number, which is 6.022 x 10^23 molecules/mol.

Number of molecules = n(O2) * Avogadro's number
= 0.179 * 6.022 x 10^23
= 1.08 x 10^23 molecules

For NH3 (ammonia gas), we have 1 liter. Using the same process as above, we can calculate the number of molecules in NH3.

n(NH3) = V(NH3) / V(molar_NH3)
= 1 L / 22.4 L/mol
= 0.045 moles

Number of molecules = n(NH3) * Avogadro's number
= 0.045 * 6.022 x 10^23
= 2.71 x 10^22 molecules

For Cl2 (chlorine gas), we have 2 liters.

n(Cl2) = V(Cl2) / V(molar_Cl2)
= 2 L / 22.4 L/mol
= 0.089 moles

Number of molecules = n(Cl2) * Avogadro's number
= 0.089 * 6.022 x 10^23
= 5.36 x 10^22 molecules

For He (helium gas), we have 8 liters.

n(He) = V(He) / V(molar_He)
= 8 L / 22.4 L/mol
= 0.357 moles

Number of molecules = n(He) * Avogadro's number
= 0.357 * 6.022 x 10^23
= 2.15 x 10^23 molecules

For CO2 (carbon dioxide gas), we have 4 liters.

n(CO2) = V(CO2) / V(molar_CO2)
= 4 L / 22.4 L/mol
= 0.179 moles

Number of molecules = n(CO2) * Avogadro's number
= 0.179 * 6.022 x 10^23
= 1.08 x 10^23 molecules

Comparing the number of molecules, we see that 4 liters of O2 contains the same total number of molecules as 4 liters of CO2.