Exciting Chemistry Question: Which Sample Contains the Most Molecules?

Which sample contains the most molecules: 1.00L of O2 at STP, 1.00L of air at STP, or 1.00L of H2 at STP?

Final answer: All the samples are equal in volume and at the same temperature and pressure (STP). So the sample with the most molecules will be the one with the smallest molecular weight, which is Hydrogen (H2). Hence, 1.00L of H2 at STP contains the most molecules.

Answer:

The sample that contains the most molecules will be the one with the smallest molecular weight. This is based on Avogadro's law, which states that equal volumes of all gases, at the same temperature and pressure, have the same number of molecules. In this case, all samples are 1.00L and at STP (Standard Temperature and Pressure).

The molecules of Hydrogen (H2) have the smallest molecular weight (about 2 g/mol), air has an average molecular weight of about 29 g/mol (because it is a mixture of several gases) and Oxygen (O2) has a molecular weight of 32 g/mol.

So, 1.00L of H2 at STP contains the most molecules.

Explanation:

The sample that contains the most molecules will be the one with the smallest molecular weight. This is based on Avogadro's law, which states that equal volumes of all gases, at the same temperature and pressure, have the same number of molecules. In this case, all samples are 1.00L and at STP (Standard Temperature and Pressure).

The molecules of Hydrogen (H2) have the smallest molecular weight (about 2 g/mol), air has an average molecular weight about 29 g/mol (because it is a mixture of several gases) and Oxygen (O2) has a molecular weight of 32 g/mol.

Therefore, 1.00L of H2 at STP contains the most molecules due to its smallest molecular weight, as per Avogadro's law.