The lattice enthalpy ΔHlatt , of magnesium bromide is 2421 kJ mol-1. Using section 20 of the data booklet and your answer to part c), determine the enthalpy of solution, ΔHsol , in kJ mol-1 of magnesium bromide.
The enthalpy of hydration for the calcium ion , ΔHhyd(Ca2+) , is 1616 kJ mol-1 . Explain why this value is less exothermic than the value for the enthalpy of hydration for the magnesium ion , ΔHhyd(Mg2+).
Use your answer to part b) and the lattice enthalpy of silver fluoride, ΔHlatt(AgF) , in section 18 in the data booklet to determine the enthalpy of formation of silver fluoride, ΔHf(AgF), in kJ mol-1.
A student added 50.00 cm3 of 1.50 mol dm-3 copper sulfate solution, CuSO4 (aq), to the polystyrene cup. They recorded the temperature every minute for 3 minutes. On the fourth minute, 6.00 g of powdered zinc was added. They then recorded the temperature of the reaction mixture every minute for a further 7 minutes. The maximum temperature change was estimated to be 29.0 °C.
Use section 6 of the data booklet to answer the following questions.
i)
Determine the amount, in moles, of copper sulfate used in the reaction.
[1]
ii)
Determine the amount, in moles, of powdered zinc used in the reaction.
