Consider this equation for the heated decomposition of potassium chlorate: 2KClO↓3(s) > 2KCl(s) + 3O↓2(g), ΔH = ?

Given these enthalpy of formation values:

KClO3: ΔHf = -391kJ/mol; KCl: ΔHf = -433kJ/mol

Calculate the enthalpy of the above reaction in kilojoules per mole of reactant.
Reference: ΔH = sum(HΔproducts) - sum(ΔHreactants)

The activity series is shown in the attached picture. if the element is below the other, then you can displace the other. following the activity series as a guide, the reactions are as follows: nickel and aluminum chloride3 ni + 2 alcl₃  → 3 nicl₂ + 2 albarium and copper bromideba + cubr  →  no reaction because cu is less oxidizable than bapotassium nitrate and aluminum3 kno₃ + al  → al(no₃)₃ + 3 ksodium phosphate and zincnaso₄ + zn  → znso₄ + na