Chemical Reactions in Chemistry
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Study Notes

Chemical Reactions

  • Chemical reactions involve the rearrangement of atoms to form new substances.
  • Reactants are the substances that undergo change.
  • Products are the substances formed in the reaction.
  • Chemical reactions are represented using chemical equations.

Evidence of a Chemical Reaction

  • The formation of a precipitate (a solid that forms and settles out of a solution).
  • The evolution of a gas (bubbles or fizzing).
  • The absorption or release of energy (change in temperature).
  • The change in color.
  • The production of a new odor.

Types of Chemical Reactions

  • Synthesis: Two or more substances combine to form a more complex substance.

    • Example: 2H₂ + O₂ → 2H₂O (water formation)
    • Requires more energy to combine into a new substance which may make heat or light released
  • Decomposition: A complex substance breaks down into two or more simpler substances.

    • Example: 2H₂O → 2H₂ + O₂ (water decomposition)
    • Requires energy put into the substance for it break down into more simple substances.
  • Single Replacement: One element replaces another element in a compound.

    • Example: Zn + 2HCl → ZnCl₂ + H₂ (zinc replaces hydrogen)
    • Generally one metal replaces another in a compound, or non-materals replaces each other in a compound.
  • Double Replacement: The positive and negative ions of two compounds exchange places.

    • Example: Na₂SO₄ + BaCl₂ → BaSO₄ + 2NaCl (exchange of ions to create a precipitate and a new substance)
    • Involves the exchange of positive and negative ions from two compound reacting with each other.

Balancing Chemical Equations

  • Chemical equations must be balanced to obey the Law of Conservation of Mass.
  • The number of atoms of each element must be equal on both sides of the equation.
    • To balance equations, use coefficients. Coefficients multiply all the subscripts in a formula.

Factors Affecting the Rate of Reaction

  • Concentration: Higher concentration of reactants leads to more collisions and a faster reaction rate.
  • Temperature: Higher temperature increases the kinetic energy of particles, leading to more frequent and energetic collisions, increasing the rate.
  • Surface Area: A greater surface area of a solid reactant increases the amount exposed to the other reactant and increases the number of collisions and subsequently the rate.
  • Catalysts: Catalysts speed up reactions by providing an alternate pathway with lower activation energy. Catalysts are not consumed in the reaction.

Energy Changes in Reactions

  • Exothermic Reactions: Reactions that release energy (often as heat) to the surroundings.
    • Example: Combustion reactions
  • Endothermic Reactions: Reactions that absorb energy from the surroundings.
    • Example: Photosynthesis in plants which needs energy from sunlight

Measuring Reaction Rates

  • Reaction rates are measured by determining the change in concentration of reactants or products over time.
  • Factors affect the observed rate
  • Reaction rates are important for understanding kinetics, and determining how fast reactions occur, and how these rates can be adjusted.

The Chemistry of Everyday Life

  • Reactions that occur commonly in our everyday lives are seen and observed quite regularly

Activation Energy

  • Activation Energy is the minimum energy required for a reaction to occur

Chemical Equations and Stoichiometry

  • Stoichiometry deals with the calculations of the quantities of reactants and products in a chemical reaction.
  • Balancing reactions is an important step in making stoichiometry calculations

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Description

Explore the fundamentals of chemical reactions, including the rearrangement of atoms, types of reactions, and signs indicating a reaction has occurred. This quiz covers crucial concepts such as synthesis, decomposition, and the evidence of chemical changes.

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