At standard temperature and pressure (STP), which statement is true about 1.00 mol samples of H2(g) and N2(g)?

• A. N2(g) occupies a larger volume than H2(g).
• B. Both samples occupy the same volume.
• C. H2(g) occupies a larger volume than N2(g).
• D. The samples have different numbers of molecules.

Answer: (B)

Verified step by step guidance

1. Recall the definition of standard temperature and pressure (STP), which is 0°C (273.15 K) and 1 atm pressure.
2. Understand that at STP, one mole of any ideal gas occupies the same volume, known as the molar volume, approximately 22.4 liters.
3. Recognize that both H2(g) and N2(g) are gases and can be approximated as ideal gases under these conditions.
4. Apply Avogadro's law, which states that equal moles of gases at the same temperature and pressure occupy equal volumes.
5. Conclude that since both samples have 1.00 mol, they must occupy the same volume and contain the same number of molecules (Avogadro's number), regardless of the gas identity.