Statement 1: Hydrogen gas $(H_{2})$ is considered a perfectly ideal gas.
Statement 2: Hydrogen atoms interact with each other via hydrogen bonds.

Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.

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Both Statement 1 and Statement 2 are correct, but Statement 2 is NOT the correct explanation of Statement 1.

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Statement 1 is correct, but Statement 2 is not correct.

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Both the Statement 1 and Statement 2 are not correct.

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Solution

The correct option is D Both the Statement 1 and Statement 2 are not correct.
The gas which has zero intermolecular forces and zero molecular volume is called as perfect ideal gas. In the case of hydrogen, the conditions for an ideal gas are not satisfied. Therefore, $H_{2}$ gas is not a perfectly ideal gas.
Also, the hydrogen bond is formed between a less electronegative hydrogen atom and more electronegative $O, N, a n d F$ .
Thus, hydrogen atoms do not interact with each other via hydrogen bonds.

Thus the correct answer is (D) Both the Statement 1 and Statement 2 are not correct.

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Statement 1: Hydrogen gas (H2) is considered a perfectly ideal gas. Statement 2: Hydrogen atoms interact with each other via hydrogen bonds.

Statement 1: Hydrogen gas $(H_{2})$ is considered a perfectly ideal gas.
Statement 2: Hydrogen atoms interact with each other via hydrogen bonds.