Answer:
Oxygen.
Explanation:
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In this case, since the ideal gas equation allows us to compute the moles of oxygen in 5.60 L at STP (1 atm and 273.15 K) as shown below:
[tex]PV=nRT\\\\n=\frac{PV}{RT}=\frac{1atm*5.60L}{0.08206\frac{atm*L}{mol*K}*273.15K}\\\\n_{O_2}= 0.25mol[/tex]
Next, given the molar mass of carbon dioxide (44.01 g/mol) we compute the moles in 10.0g of this gas via:
[tex]n_{CO_2}=10.0gCO_2*\frac{1molCO_2}{44.01gCO_2} =0.23molCO_2[/tex]
Thus, since oxygen has the greatest number of moles, we immediately infer it also has the greatest number of molecules based on the Avogadro's number.
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