According to Boyle’s Law, if the pressure of a gas is doubled, what happens to its volume?

The volume of the gas is halved, since pressure and volume are inversely proportional.

Fill in the blank: When the absolute temperature of a gas increases at constant pressure, its volume ___ .

Increases

What is the standard temperature in Kelvin used in gas law calculations?

273 K

True or False: Gay-Lussac’s law states that the volume of a gas is directly proportional to its temperature at constant pressure.

False; it states that pressure is directly proportional to temperature at constant volume.

Calculate the relative molecular mass of a gas with a vapor density of 18.

The relative molecular mass is 2 × 18 = 36.

What is the molecular formula for a gas if its empirical formula is CH₂ and its molar mass is 42 g/mol?

C₃H₆, since the empirical formula mass is 14 g/mol, and 42 g/mol / 14 g/mol = 3.

Fill in the blank: Avogadro’s Law states that equal volumes of gases at the same temperature and pressure contain ___ .

Equal numbers of molecules

If a gas has an atomicity of 4, what is the molecular formula for this gas?

The molecular formula is X₄, where X is the element.

True or False: Diatomic gases consist of two different atoms.

False; diatomic gases consist of two identical atoms.

What is the relationship between molecular mass and vapor density as per the gas laws?

Relative vapor density is equal to the relative molecular mass divided by 2.

Calculate the empirical formula mass of C₆H₁₂O₆.

The empirical formula mass is 6(12) + 12(1) + 6(16) = 180 g/mol.

Fill in the blank: The ratio of reacting gases according to Gay-Lussac’s law can be expressed in simple ___ .

Whole number ratios

What is the term for the mass of one mole of a substance, expressed in grams?

Molar mass

If the empirical formula of a compound is NH₂ and its molecular formula has a molar mass of 32 g/mol, what is the molecular formula?

N₂H₄, since the empirical formula mass is 16 g/mol and 32 g/mol / 16 g/mol = 2.

True or False: The empirical formula provides the exact number of atoms of each element in a molecule.

False; the empirical formula shows the simplest ratio of elements in a compound.