10 dm^3 of N_2 gas and 10 dm^3 of gas X at | vedclass

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(A) According to Avogadro's Law,equal volumes of all gases at the same temperature and pressure contain an equal number of molecules.Since both gases

Vedclass · Accepted Answer

$CO$

Vedclass · Answer

(A) According to Avogadro's Law,equal volumes of all gases at the same temperature and pressure contain an equal number of molecules.Since both gases occupy the same volume $(10 \ dm^3)$ at the same temperature and pressure,they must contain the same number of moles.For the number of molecules to be identical,the molar mass of gas $X$ must be equal to the molar mass of $N_2$ if the masses were equal,or simply,the gases must have the same molecular weight if they are diatomic with the same number of atoms.The molar mass of $N_2 = 2 	imes 14 = 28 \ g/mol$.Checking the options:$A$: $CO = 12 + 16 = 28 \ g/mol$.$B$: $CO_2 = 12 + 32 = 44 \ g/mol$.$C$: $H_2 = 2 	imes 1 = 2 \ g/mol$.$D$: $NO = 14 + 16 = 30 \ g/mol$.Therefore,the gas $X$ is $CO$.

$10 \ dm^3$ of $N_2$ gas and $10 \ dm^3$ of gas $X$ at the same temperature and pressure contain the same number of molecules. The gas $X$ is

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