At room temperature and pressure, syringe A contains 24 cm324\,\mathrm{cm^{3}}24cm3 of hydrogen and syringe B contains 24 cm324\,\mathrm{cm^{3}}24cm3 of carbon dioxide. One mole of hydrogen has a mass of 2.0 g and one mole of carbon dioxide has a mass of 44.0 g.
Which statement correctly compares the amounts and masses of gas in the syringes?
The samples contain the same amount in moles, but syringe B contains a greater mass.
Each syringe contains one mole, but syringe B contains a greater mass.
Syringe B contains a greater amount in moles and a greater mass than syringe A.
Syringe A contains a greater amount in moles, but syringe B contains a greater mass.
152 exam-style questions on OCR GCSE Chemistry 5.1 Monitoring chemical reactions, covering 5.1.1 The technique of titration, 5.1.2 Theoretical mass, percentage yield and atom economy, 5.1.3 Concentration of a solution in mol/dm3, 5.1.4 Concentration calculations and titration results, 5.1.5 Molar gas volume and volumes of gases in reactions, and 5.1.6 Choosing a reaction pathway. Each one has a worked solution and a mark scheme showing where the marks go.