Conservation Of Mass And Balanced Chemical Equations (GCSE Chemistry)

In a titration, 25.00 cm3 of a sodium hydroxide solution is neutralised by 30.00 cm3 of 0.100 mol/dm3 HCl. What is the concentration of NaOH?

When 2.00 mol of hydrogen reacts completely with 1.00 mol of oxygen to form water, what mass (g) of water is produced? (Mr H2O = 18.0)

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

Ammonia (NH3) reacts with oxygen to make nitric oxide and water: 4 NH3 + 5 O2 ? 4 NO + 6 H2O. How many moles of O2 are needed to react with 2.0 mol NH3?

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:

What is the empirical formula of a compound that is 40.0% C, 6.7% H, 53.3% O by mass (approx)?

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

Which set of quantities is needed to calculate the mass of product formed from a given mass of reactant using reacting masses?

An element X forms an oxide X2O3. If 2.00 g of X combine with 0.48 g oxygen, what is the relative atomic mass (Ar) of X (approx)?

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 0.250 mol of NaCl is dissolved in enough water to make 0.500 dm3 of solution, what is the concentration in mol/dm3?