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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

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The number of molecules is the same in both gases.

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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 have the same volume $(1 \, cm^3)$ at $N.T.P$,the number of molecules is the same in both.The internal energy of an ideal gas depends only on its temperature $(U = \frac{f}{2} nRT)$. Since both gases are at the same temperature and have the same number of moles (due to equal volume at $N.T.P$),their internal energies are the same.The average velocity (root mean square velocity) of gas molecules is given by $v_{rms} = \sqrt{\frac{3RT}{M}}$. Since the molar mass $(M)$ of hydrogen $(H_2)$ and oxygen $(O_2)$ are different,their average velocities will be different. Therefore,statement $B$ is incorrect.Since statement $B$ is incorrect,statement $D$ is also incorrect. Thus,both $A$ and $C$ are technically correct,but in the context of standard multiple-choice questions,the most fundamental property derived from $N.T.P$ conditions is the number of molecules.

Hydrogen gas and oxygen gas have a volume of $1 \, cm^3$ each at $N.T.P$. Which of the following statements is correct?

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