Using the molar volume in calculations with chemical equations

Calculate the number of moles in 360 cm³ of nitrogen gas at room temperature and pressure. Give your answer to two decimal places. (Molar volume = 24,000 cm³ at rtp)

A student needs to calculate the mass of carbon dioxide produced when 48,000 cm³ of carbon dioxide is collected at room temperature and pressure. Explain the steps, including the formulae needed, to calculate the mass of carbon dioxide produced. (Ar: C = 12, O = 16; molar volume = 24,000 cm³ at rtp)

The table below shows the volumes, in cm³, of a gas collected from several reactions at room temperature and pressure. Fill in the number of moles of gas for each row, using the molar volume of 24,000 cm³ at rtp.

Which calculation gives the number of moles of a gas from its volume at rtp (using cm³)?

Calculate the volume, in dm³, of chlorine gas produced at rtp from the complete decomposition of 2.7 g of potassium chlorate, KClO₃. The balanced equation is:

(Ar: K = 39, Cl = 35.5, O = 16; molar volume = 24 dm³)

Ammonium nitrate decomposes to form dinitrogen oxide (N2O) and water. The balanced equation is:

A practical uses 8.0 g of ammonium nitrate. (Ar: N = 14, H = 1, O = 16; molar volume at rtp = 24 dm³)

A student collects 8.4 g of oxygen gas at room temperature and pressure (rtp). Calculate the volume, in dm³, of this oxygen gas. (Ar: O = 16; molar volume = 24 dm³ at rtp.)

When sodium nitrate (ce{NaNO3}) decomposes on heating, it produces sodium nitrite (ce{NaNO2}) and oxygen gas (ce{O2}). The equation is:

Calculate the number of moles of neon gas present in a 4.8 dm³ flask at room temperature and pressure. Give your answer to two decimal places. (Molar volume = 24 dm³ at rtp.)