R2 Reactivity 2: How much, how fast and how far?

Practice questions on Reactivity 2: How much, how fast and how far?

• Explain how an increase in temperature increases the rate of a chemical reaction, with ref… (4 marks, Explain)
• Explain how the law of conservation of mass is consistent with the concept of mole ratios … (4 marks, Explain)
• Explain how the concepts of limiting reagent and percentage yield are used together to eva… (4 marks, Explain)
• A student reacts excess zinc metal with 25.0 cm³ of 0.500 mol dm⁻³ hydrochloric acid. Afte… (4 marks, Explain)
• Explain why the theoretical yield of a product calculated from stoichiometry is almost nev… (4 marks, Explain)
• Ammonia is produced industrially by the Haber process: N₂(g) + 3H₂(g) → 2NH₃(g). In a part… (4 marks, Explain)
• Explain how the addition of a small amount of concentrated hydrochloric acid to an aqueous… (4 marks, Explain)
• Explain why increasing the concentration of a reactant in solution increases the rate of a… (4 marks, Explain)
• For the equilibrium N₂(g) + 3H₂(g) ⇌ 2NH₃(g), explain how an increase in total pressure at… (4 marks, Explain)
• Explain how a catalyst increases the rate of a chemical reaction, with reference to activa… (4 marks, Explain)
• Explain why the rate of a gas-phase reaction increases when the pressure is increased at c… (4 marks, Explain)
• Explain how the Maxwell–Boltzmann distribution of molecular energies can be used to accoun… (4 marks, Explain)
• Explain why the value of the equilibrium constant, Kc, for a reversible reaction changes w… (4 marks, Explain)
• A student claims that adding a catalyst to a reaction mixture at equilibrium will increase… (4 marks, Evaluate)
• A saturated aqueous solution of calcium fluoride, CaF₂, is in equilibrium with excess undi… (4 marks, Explain)