One liter of oxygen gas at standard temperature and pressure has a mass of 1.43 g. The same volume of hydrogen gas under these conditions is 0.089 g. If both volumes contain the same number of gas particles (according to Avogadro's hypothesis), how can this difference in mass be explained?

Indeed, the two samples should contain about the same number of gas particles. However, the molar mass of is larger than that of (by a factor of about .) Therefore, the mass of the sample is significantly larger than that of the sample.

Explanation:

The and the sample here are under the same pressure and temperature, and have the same volume. Indeed, if both gases are ideal, then by Avogadro's Law, the two samples would contain the same number of gas particles ( and molecules, respectively.) That is:

.

Note that the mass of a gas is different from the number of gas particles in it. In particular, if all particles in this gas have a molar mass of , then:

.

In other words,

The ratio between the mass of the and that of the sample would be:

.

Since by Avogadro's Law:

.

Look up relative atomic mass data on a modern periodic table:

Therefore:

Verify whether :

Note that the mass of the sample comes with only two significant figures. The two sides of this equations would indeed be equal if both values are rounded to two significant figures.

water and alcohols have similar properties because water molecules contain hydroxyl groups that can form hydrogen bonds with other water molecules and with alcohol molecules, and likewise alcohol molecules can form hydrogen bonds with other alcohol molecules as well as with water.