In the laboratory, 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. Reactants can be elements or compounds. In this case it is a gas and a metal which will react and produce a compound. The general form of a synthesis reaction is A + B → AB. For this lab to be successful, you need knowledge of percent composition, empirical and molecular formula, law of conservation of mass, moles and molar mass, qualitative and quantitative. To begin, the composition percentage of a compound is the percentage of the total mass of each element in that compound. Each compound would have a certain percentage composition. To calculate the percentage composition of a compound, you must determine the total molecular mass of the compound. For example, for H2O, the total molar mass would be 18.00 g/mol. You then need to enter the mass of one of the elements and the molar passage into the equation wt% (mass) of element = (total mass of element present ÷ total mass of compound) x 100 to find out the composition percentage. So for oxygen, it would be %O = (16.00 g ÷ 18.00 g/mol) x 100, which would be 88.9%. Therefore, the percentage composition of O in this compound is approximately 88.9%. Additionally, the molecular formula is the number and types of atoms that exist in a single molecule of a substance. The empirical formula also known as the simplest formula is the ratio of the elements present in the compound. The main difference between these two elements is that the empirical formula shows the simplest positive integer ratio of the atoms of each element present in a compound, whereas the molecular formula of a compound is a way...... in the middle paper.....arbon. One mole of water would have a molar mass of 18 g/mol (H2O molar mass: (1.008x2) + 16.00 = 18.016 g/mol). Additionally, the law of conservation of mass was first established in 1789 by a French chemist named Antoine Lavoisier. The law states that mass is neither created nor destroyed in an 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). For example, 1.00 g of carbon + 5.34 g of sulfur = 6.34 g of carbon disulfide. In any chemical reaction, the mass of the objects produced will be the same as that of the reactant used. The mass of things reacted is equal to the mass of things produced. So if you react 1 kg of substance, the result will also be 1 kg of substance. Materials do not “disappear” and other materials are not “created”. This applies because mass cannot be created or destroyed..