Mass in a chemical reaction: using moles (RAM 1 d.p.)

12 questions

1. Given the relative atomic masses (Ar): C (12.0), O (16.0).Calculate the relative formula mass (Mr) of carbon dioxide (CO₂).
2. What does the conservation of mass in a chemical reaction imply?
3. If 20 g of sodium reacts fully with 15 g of chlorine, how much sodium chloride is produced?
4. For the equation __ N₂ + __ H₂ → __ NH₃, select the correct coefficients to balance it.
5. What does the equation 2H₂ + O₂ → 2H₂O tell us?
6. Given the relative atomic mass values (Ar): H (1.0), S (32.1), O (16.0).Calculate the relative formula mass (Mr) of sulfuric acid.
7. What does stoichiometry mean in chemistry?
8. In a balanced chemical equation, what does the mole ratio of reactants and products tell us?
9. The ___ is the sum of the relative atomic masses of all the atoms in a formula, representing the mass of a molecule relative to the mass of a carbon-12 atom.
10. Which of the following statements best describes what the equation 2H₂ + O₂ → 2H₂O tells us?
11. Given the reaction: CH₄ + 2O₂ → CO₂ + 2H₂O, how many grams of CO₂ are produced when 16 g of methane (CH₄) reacts completely? Relative formula mass values: (CH₄ = 16.0) and (CO₂ = 44.0)
12. Using the reaction: N₂ + 3H₂ → 2NH₃, calculate the mass of ammonia (NH₃) produced when 14 g of nitrogen react with hydrogen? (2 s.f.)Relative formula mass values: (N₂ = 28.0) & (NH₃ = 17.0)

License: OGL