Identify as diatomic element (DE) / non -diatomic element (NDE) / compound (C)(2rekmen16 etters co __ H_(2) __ MgO __ C __ CH_(4)O __ CaF_(2) __ F_(2) __ CO_(2) __ __ s H_(2)O __ compand O_(2) __ p __ E) LAW OF CONSERVATION OF MASS (Matter') MATH In 1789 Antoine Lavoisier postulated the Law of Conservation of Mass (Matter) which states that matter cannot be created nor destroyed!From this we know that all chemical equations must be BALANCED or have the same amount (mass) of reactants and products In his experiment he studied the decomposition of Mercury (II) oxide. Lavoisier's Conservation of Mass Experiment:(balance the equation) underline ( )HgO( )arrow underline ( )O_(2)( )+underline ( )Hg ( ) 10.0g=0.7g+9.3g red powder Mass of Reactants=Mass of Products

Let's identify each substance as a diatomic element (DE), non-diatomic element (NDE), or compound (C):<br /><br />1. $H_{2}$ - DE (Diatomic Element)<br />2. $MgO$ - C (Compound)<br />3. C - NDE (Non-Diatomic Element)<br />4. $CH_{4}O$ - C (Compound)<br />5. $CaF_{2}$ - C (Compound)<br />6. $F_{2}$ - DE (Diatomic Element)<br />7. $CO_{2}$ - C (Compound)<br />8. $H_{2}O$ - C (Compound)<br />9. $O_{2}$ - DE (Diatomic Element)<br /><br />For the Law of Conservation of Mass experiment, balance the equation for the decomposition of Mercury (II) oxide:<br /><br />Unbalanced: \(\underline{\quad}HgO(\quad) \rightarrow \underline{\quad}O_{2}(\quad) + \underline{\quad}Hg\quad(\quad)\)<br /><br />Balanced: \(2HgO(s) \rightarrow O_{2}(g) + 2Hg(l)\)<br /><br />This balanced equation reflects that the mass of reactants equals the mass of products, consistent with the Law of Conservation of Mass.