Questions and Answers
What is the primary characteristic that distinguishes a chemical reaction from a physical change?
Change in chemical composition
Which of the following is an example of a combustion reaction?
2CH4 + 3O2 → 2CO2 + 3H2O
What is the purpose of coefficients in a chemical reaction equation?
To balance the equation
Which of the following factors can affect the rate of a chemical reaction?
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What is the term for a substance that speeds up a chemical reaction without being consumed?
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In a chemical reaction equation, what is written on the left side of the equation?
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What is the term for a reaction in which a single reactant breaks down into two or more products?
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What is the principle that states that the total mass of the reactants equals the total mass of the products?
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Which of the following is an example of a synthesis reaction?
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What is the term for a reaction in which one element or group of elements replaces another element or group of elements in a compound?
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Study Notes
Chemical Reaction
A chemical reaction is a process in which one or more substances (reactants) are converted into new substances (products).
Types of Chemical Reactions:
-
Synthesis Reaction: Two or more reactants combine to form a single product.
- Example: 2H2 + O2 → 2H2O
-
Decomposition Reaction: A single reactant breaks down into two or more products.
- Example: 2H2O → 2H2 + O2
-
Replacement Reaction: One element or group of elements replaces another element or group of elements in a compound.
- Example: Zn + CuSO4 → ZnSO4 + Cu
-
Combustion Reaction: A reaction between a substance and oxygen, resulting in heat and light.
- Example: 2CH4 + 3O2 → 2CO2 + 3H2O
Characteristics of Chemical Reactions:
- Chemical Change: A change in the chemical composition of the reactants.
- Conservation of Mass: The total mass of the reactants equals the total mass of the products.
- Energy Change: Chemical reactions often involve the absorption or release of energy.
Factors Affecting Chemical Reactions:
- Concentration: The amount of reactants present can affect the rate of reaction.
- Temperature: An increase in temperature can increase the rate of reaction.
- Pressure: An increase in pressure can increase the rate of reaction.
- Catalysts: Substances that speed up chemical reactions without being consumed.
Chemical Reaction Equations:
- Reactants: Written on the left side of the equation.
- Products: Written on the right side of the equation.
- Arrow: Indicates the direction of the reaction.
- Coefficients: Numbers in front of formulas to balance the equation.
Chemical Reaction
- A process in which one or more substances (reactants) are converted into new substances (products)
Types of Chemical Reactions
- Synthesis Reaction: two or more reactants combine to form a single product, example: 2H2 + O2 → 2H2O
- Decomposition Reaction: a single reactant breaks down into two or more products, example: 2H2O → 2H2 + O2
- Replacement Reaction: one element or group of elements replaces another element or group of elements in a compound, example: Zn + CuSO4 → ZnSO4 + Cu
- Combustion Reaction: a reaction between a substance and oxygen, resulting in heat and light, example: 2CH4 + 3O2 → 2CO2 + 3H2O
Characteristics of Chemical Reactions
- Chemical Change: a change in the chemical composition of the reactants
- Conservation of Mass: the total mass of the reactants equals the total mass of the products
- Energy Change: chemical reactions often involve the absorption or release of energy
Factors Affecting Chemical Reactions
- Concentration: the amount of reactants present can affect the rate of reaction
- Temperature: an increase in temperature can increase the rate of reaction
- Pressure: an increase in pressure can increase the rate of reaction
- Catalysts: substances that speed up chemical reactions without being consumed
Chemical Reaction Equations
- Reactants: written on the left side of the equation
- Products: written on the right side of the equation
- Arrow: indicates the direction of the reaction
- Coefficients: numbers in front of formulas to balance the equation
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