Law of Conservation of Matter and Balancing Equations

Law of Conservation of Matter

• Definition: Matter is neither created nor destroyed.
  • If ash appears less massive than the original wood or coal, it's because the fumes escaped.

Mass Conservation in Chemical Equations

• The total mass of the reactants must equal the total mass of the products.
• This principle explains why we balance chemical equations.
• We cannot create mass from nothing or destroy it during a chemical reaction.

The Origin of Matter: Einstein's Equation

• Question: If mass cannot be created, how did it originate?
• Answer: Matter arises from energy, according to Einstein's equation: E = mc^2
  • Where:
    • E = Energy
    • m = Mass
    • c = Speed of light

String Theory and Membranes (Brains)

• One theory suggests that matter arises from energy through membranes and string theory.
• At a certain stability point (around three), matter can arise.
• Beyond that, higher dimensions may emerge

Atomic Mass Units (AMU)

• Each element has its mass number, representing AMU per atom.
• It's simpler to count atoms of each element rather than converting AMU to kilograms.

Counting Atoms

• The number of atoms of each element must be the same on both the reactant and product sides of a chemical equation.
• Example: H_2O means two hydrogen atoms and one oxygen atom.

Subscripts and Coefficients

• Subscripts indicate the number of atoms of an element in a compound.
  • Example: In CH_4 (methane), there is one carbon atom and four hydrogen atoms.
• Coefficients are used to balance equations without changing the identity of the reactants or products.
  • They are placed in front of the chemical formulas, similar to coefficients in algebraic equations.
  • Example: If you have 2CH_4, you have 2
    eq 1 = 2 carbon atoms and 2
    eq 4 = 8 hydrogen atoms.