1) No reaction. Both possible products, AgNO₃ and Na₂SO₄, are soluble in water, so no precipitate forms to drive a double displacement reaction.
2) No reaction. Sodium iodide (NaI) and calcium sulfate (CaSO₄) are both soluble ionic compounds. A double displacement reaction would produce Na₂SO₄ and CaI₂, both of which are also soluble, so no precipitate, gas, or water forms to drive the reaction.
3) 2 HNO₃ + Ca(OH)₂ → Ca(NO₃)₂ + 2 H₂O. This is an acid-base neutralization reaction producing soluble calcium nitrate and water.
4) CaCO₃ → CaO + CO₂. This is a decomposition reaction (thermal decomposition) that occurs upon heating.
5) AlCl₃ + (NH₄)₃PO₄ → AlPO₄ + 3 NH₄Cl. This is a double displacement reaction where aluminum phosphate (AlPO₄) precipitates as it is insoluble, while ammonium chloride (NH₄Cl) remains dissolved.
6) No reaction. Lead (Pb) is less reactive than iron (Fe) according to the activity series. Therefore, lead cannot displace iron from its compound, Fe(NO₃)₃.
7) 2 C₃H₆ + 9 O₂ → 6 CO₂ + 6 H₂O. This is a combustion reaction of propene, producing carbon dioxide and water.
8) No reaction. Sodium metal (Na) is highly reactive, but calcium sulfate (CaSO₄) is not a typical reactant for single displacement with metals because it is only sparingly soluble and the calcium ion is not easily displaced by sodium in aqueous solution. Furthermore, sodium reacts violently with water, but CaSO₄ does not provide a suitable environment for this specific displacement.
Parent Tip: Review the logic above to help your child master the concept of predicting the products of chemical reactions worksheet.
