The Law of Conservation of Matter

We’ve talked about changes in matter… The evaporation of a puddle of water Rust forming on a metal fence PHYSICAL CHEMICAL

HOWEVER… No matter is created or destroyed by such changes! The total amount of matter remains constant.

The Law of Conservation of Matter During a chemical reaction, matter cannot be created or destroyed it can only change forms. Even though the matter may change from one form to another, the same number of atoms exists before and after the change takes place!

Since the overall mass of the matter does not change… The mass of the reactants – the substances there before the reaction occurs – must equal the mass of the product – the substances there after the reaction takes place. Mass of Reactants Mass of Products

An Example of the L.C.M. Test tube containing lead nitrate is placed upright in a flask that contains potassium iodide. What are these? REACTANTS! They don’t mix!

A stopper is put in place to create a closed system – an environment where matter cannot enter or escape. The mass of the system is found.

After the mass is found, the system is turned upside down so the lead nitrate can mix with the potassium iodide. They create lead iodide and potassium nitrate.

Although the matter changed in form, the total mass of the system remains unchanged.

The Formation of Rust Iron Rust Hard, gray-colored metal Flaky, orange-red solid

When iron reacts with oxygen in the air, they form rust or IRON OXIDE. This is written as: Iron + Oxygen Iron Oxide

TAKE A LOOK AT THE NUMBERS Each made of TWO oxygen atoms Fe Fe O2 Fe2O3 Fe2O3 Fe Fe O2 O2 What about the PRODUCT? How many Oxygen atoms? How many Iron atoms? PRODUCT REACTANTS

All Chemical Reactions follow the Law of Conservation of Matter With Iron Oxide, the MASS STAYS THE SAME! The total number of iron atoms and oxygen atoms in the reactants is the same as that in the product. The atoms were just rearranged! No new atoms were created and none were destroyed!

Determining the Mass of Reactants and Products REMEMBER: The mass of the reactants is always equal to the mass of the products. Mass of Reactants Mass of Products

Example: Tin Fluoride Tin + hydrogen fluoride -> tin fluoride + hydrogen What’s the total mass of the reactants? 158.72 g So what should the mass of the products be? 118.7 g 40.02 g

Balancing Chemical Equations Demonstrating the Law of Conservation of Matter

What is a chemical equation? Chemical equation - Describes a chemical change. Parts of an equation: Reactant Product 2Ag + H2S Ag2S + H2 Reaction symbol

Reactants and Products Reactant - The chemical(s) you start with before the reaction. Written on left side of equation. Product - The new chemical(s) formed by the reaction. Right side of equation.

Subscripts and Coefficients Subscript - shows how many atoms of an element are in a molecule. EX: H2O 2 atoms of hydrogen (H)‏ 1 atom of oxygen (O)‏ Coefficient - shows how many molecules there are of a particular chemical. EX: 3 H2O Means there are 3 water molecules.

A Chemical Reaction 2H2 + O2 → 2H2O

Law of Conservation of Mass In a chemical reaction, matter is neither created nor destroyed. In other words, the number and type of atoms going INTO a reaction must be the same as the number and type of atoms coming OUT. If an equation obeys the Law of Conservation of Matter, it is balanced.

A Balanced Equation CH4 + 2O2 → CO2 + 2H2O Reactant Side Product Side 1 carbon atom 4 hydrogen atoms 4 oxygen atoms 1 carbon atom 4 hydrogen atoms 4 oxygen atoms

An Unbalanced Equation CH4 + O2 → CO2 + H2O Reactant Side Product Side 1 carbon atom 4 hydrogen atoms 2 oxygen atoms 1 carbon atom 2 hydrogen atoms 3 oxygen atoms