Types of Chemical Reactions

Synthesis Reaction: Two or more substances combine to form a new compound.
- Example: 2H2 + O2 → 2H2O
Decomposition Reaction: A single compound breaks down into two or more substances.
- Example: 2H2O → 2H2 + O2
Replacement Reaction: One element replaces another element in a compound.
- Example: Zn + CuSO4 → ZnSO4 + Cu
Combustion Reaction: A substance reacts with oxygen to produce heat and light.
- Example: 2CH4 + 3O2 → 2CO2 + 3H2O
Neutralization Reaction: An acid reacts with a base to form a salt and water.
- Example: HCl + NaOH → NaCl + H2O

A chemical equation is a representation of a chemical reaction using chemical formulas and symbols.
The reactants are written on the left side of the equation, and the products are written on the right side.
The arrow (→) separates the reactants from the products.
Chemical equations can be balanced by adding coefficients in front of the reactants or products.

Factors Affecting Reaction Rate:
- Concentration: Increasing the concentration of reactants increases the reaction rate.
- Temperature: Increasing the temperature increases the reaction rate.
- Surface Area: Increasing the surface area of reactants increases the reaction rate.
- Catalyst: Adding a catalyst can increase the reaction rate.
Reaction Rate Expression: A mathematical expression that describes the rate of a chemical reaction.

Elementary Reaction: A single step in a chemical reaction mechanism.
Reaction Intermediate: A molecule that forms during a chemical reaction but is not a reactant or product.
Rate-Determining Step: The slowest step in a chemical reaction mechanism, which determines the overall rate of the reaction.

Catalyst: A substance that increases the reaction rate without being consumed by the reaction.
Inhibitor: A substance that decreases the reaction rate.
Activation Energy: The minimum energy required for a chemical reaction to occur.
Pressure: Increasing the pressure can increase the reaction rate.
Light: Certain reactions can be affected by light.

A synthesis reaction involves two or more substances combining to form a new compound, e.g., 2H2 + O2 → 2H2O.
A decomposition reaction involves a single compound breaking down into two or more substances, e.g., 2H2O → 2H2 + O2.
A replacement reaction involves one element replacing another element in a compound, e.g., Zn + CuSO4 → ZnSO4 + Cu.
A combustion reaction involves a substance reacting with oxygen to produce heat and light, e.g., 2CH4 + 3O2 → 2CO2 + 3H2O.
A neutralization reaction involves an acid reacting with a base to form a salt and water, e.g., HCl + NaOH → NaCl + H2O.

A chemical equation represents a chemical reaction using chemical formulas and symbols.
Reactants are written on the left side of the equation, while products are written on the right side.
The arrow (→) separates the reactants from the products.
Chemical equations can be balanced by adding coefficients in front of the reactants or products.

Factors that affect reaction rates include concentration, temperature, surface area, and catalysts.
Increasing concentration, temperature, and surface area can increase reaction rates.
Adding a catalyst can also increase the reaction rate.
The reaction rate expression is a mathematical description of the reaction rate.

An elementary reaction is a single step in a chemical reaction mechanism.
A reaction intermediate is a molecule that forms during a chemical reaction but is not a reactant or product.
The rate-determining step is the slowest step in a chemical reaction mechanism, which determines the overall reaction rate.

A catalyst is a substance that increases the reaction rate without being consumed by the reaction.
An inhibitor is a substance that decreases the reaction rate.
Activation energy is the minimum energy required for a chemical reaction to occur.
Increasing pressure and certain wavelengths of light can also impact reaction rates.

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