# Matter Cannot Be Created or Destroyed, Only Transformed from One Form to Another

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In the lab the reaction that took place was a synthesis reaction. A synthesis reaction, is a type of chemical reaction in which two or more simple substances combine to form a new product. The reactants may be elements or compounds. In this case it is a gas and a metal that will react and produce a compound. The general form of a synthesis reaction is, A + B → AB. In order for this lab to be done successful you need knowledge on, percent composition, the empirical and molecular formula, the law of conservation of mass, moles and molar mass, qualitative and quantitative. To begin, the percent composition of a compound is the percent of the total mass that each element has in that compound. Every compound would have a certain percent composition. To calculate percent composition of a compound, you would have to determine the total molecular mass of the compound. For example, for H2O the total molar mass would be 18.00g/mol. You would then input the mass of one of the elements and the molar pass into the equation % by weight (mass) of element = (total mass of element present ÷ total mass of compound) x 100 to find out the percent composition. So for Oxygen it would be, % of O = (16.00g ÷ 18.00g/mol) x 100 which would equal 88.9%. Therefore the percent composition of O in this compound is roughly 88.9%. Furthermore, the molecular formula is the number and types of atoms that are existing in a single molecule of a substance. The empirical formula also known as the simplest formula is the ratio of elements present in the compound. The key difference between these two is that the empirical formula shows the simplest positive integer ratio of atoms of each element present in a compound whereas the molecular formula of a compound is a way ...

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...arbon. A mole of water would have the molar mass of 18g/mol (H2O Molar Mass: (1.008x2) + 16.00 = 18.016g/mol). Additionally, The law of conservation of mass was first established in 1789 by a French chemist name Antoine Lavoisier. The law states that mass is neither created nor destroyed in any ordinary chemical reaction. Or more simply, the mass of substances produced (products) by a chemical reaction is always equal to the mass of the reacting substances (reactants). E.g., 1.00g carbon + 5.34g sulphur = 6.34g carbon disulphide. In any chemical reaction the mass of things produced will be the same like the reactant it used. Mass of things reacted equals mass of things produced. So if you react 1 kg of stuff, the result will also be 1 kg of stuff. The materials do not "disappear" nor are other materials “created". This applies as mass cannot be created nor destroyed.

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