Question 1

The image shows two containers with equal masses and equal numbers of gas particles under identical conditions. According to Avogadro's hypothesis, what can be inferred about the volumes of the two gases if the pressure and temperature are the same?

Accepted Answer

The volumes of the two gases are the same because equal numbers of molecules at the same temperature and pressure occupy equal volumes.

Question 2

If the left container contains oxygen molecules ($$O_2) $$and the right container contains carbon dioxide molecules ($$CO_2$$), and both have the same number of molecules, which statement is correct about the mass of gas in each container?

Accepted Answer

The mass of $$CO_2 is $$greater than the mass of $$O_2$$ because $$CO_2$$ has a higher molar mass.

Question 3

If each container in the image contains 1 mol of gas at standard temperature and pressure (STP), what is the volume of gas in each container?

Accepted Answer

$$22.4 L$$

Question 4

Suppose the blue spheres represent nitrogen gas ($$N_2) $$and the brown spheres represent argon gas ($$Ar). If $$both containers have the same number of particles and are at the same temperature and pressure, which property is necessarily the same for both gases?

Accepted Answer

The volume occupied by the gases

Question 5

If the pressure and temperature are kept constant, but the number of particles in the left container is doubled, what happens to the volume of the gas according to Avogadro's Law?

Accepted Answer

The volume doubles.

Formulas, Nomenclature, and Stoichiometry in Inorganic Chemistry

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