Conservation Of Mass And Balanced Chemical Equations (GCSE Chemistry)

A solution contains 0.100 mol of HCl in 250 cm3. What is the concentration in mol/dm3?

Which statement best describes the law of conservation of mass in a chemical reaction?

A gas occupies 24.0 dm3 at room temperature and pressure (RTP). How many moles of gas does it contain?

When 100 g of calcium carbonate (CaCO3) decomposes completely to calcium oxide (CaO) and carbon dioxide (CO2) in a closed container, the mass of the products will be:

Which calculation gives the number of moles in 36.0 g of water (H2O)? (Ar H = 1, O = 16)

Which shows the correct mole ratio in the balanced equation: 2 Al + 3 Cl2 ? 2 AlCl3 ?

Calculate the relative formula mass (Mr) of calcium carbonate (CaCO3). (Ar Ca = 40.1, C = 12.0, O = 16.0)

A student mixes 8.0 g of reactant A with 12.0 g of reactant B. After the reaction finishes, 3.0 g of solid product remains plus leftover unreacted B. Which statement must be true by conservation of mass?

If a balanced equation gives a mole ratio 1:2:1 (A:B:C) and you start with 1.00 mol A and 5.00 mol B, which is limiting and how many moles of C form?

If 10.0 g of magnesium react with excess hydrochloric acid to form magnesium chloride and hydrogen, the mass of hydrogen produced (approximately) is closest to:

At RTP 1 mole of any gas occupies 24.0 dm3. If 48.0 dm3 of oxygen is collected, how many moles is that?