Suppose a 5.00 l sample of o2 at a given temperature and pressure contains 1.08

Missing question: A 5.00 L sample of O2 at a given temperature and pressure contains a 1.08x10^23 molecules. How many molecules would be contained in each of the following at the same temperature and pressure? 
a) 5.00 L H2.
b) 5.00 L CO2.
Use Avogadro's Law: The Volume Amount Law: equal volumes of all gases, at the same temperature and pressure, have the same number of molecules. Because hydrogen and carbon(IV) oxide are gases, number of molecules are the same as number of oxygen molecules, so:
a) N(H₂) = 1.08·10²³.
b) N(CO₂) = 1.08·10²³

Ithink d hope that