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Questions and Answers
What is the main process involved in a chemical reaction?
What is the main process involved in a chemical reaction?
What type of reaction involves the breaking down of a single compound into two or more substances?
What type of reaction involves the breaking down of a single compound into two or more substances?
What is the purpose of coefficients in a chemical equation?
What is the purpose of coefficients in a chemical equation?
What is the law that states that matter cannot be created or destroyed in a chemical reaction?
What is the law that states that matter cannot be created or destroyed in a chemical reaction?
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What is the study of the quantitative relationships between reactants and products in a chemical reaction?
What is the study of the quantitative relationships between reactants and products in a chemical reaction?
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What is the arrow (→) used to indicate in a chemical equation?
What is the arrow (→) used to indicate in a chemical equation?
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What should never be changed in a chemical formula?
What should never be changed in a chemical formula?
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What type of reaction is represented by the equation 2H2 + O2 → 2H2O?
What type of reaction is represented by the equation 2H2 + O2 → 2H2O?
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Study Notes
Chemical Reactions
A chemical reaction is a process that involves the transformation of one or more substances into new substances.
Types of Chemical Reactions
- Synthesis Reaction: Two or more substances combine to form a new compound.
- Decomposition Reaction: A single compound breaks down into two or more substances.
- Replacement Reaction: One element replaces another element in a compound.
- Combustion Reaction: A substance reacts with oxygen to produce heat and light.
Chemical Equations
A chemical equation represents a chemical reaction using chemical formulas and symbols.
Parts of a Chemical Equation
- Reactants: The substances that undergo a chemical change.
- Products: The substances formed as a result of the chemical reaction.
- Arrow: Indicates the direction of the reaction (→).
- Coefficients: Whole numbers that indicate the relative amounts of reactants and products.
Writing Chemical Equations
- Write the reactants on the left and products on the right.
- Use the arrow (→) to separate reactants and products.
- Use coefficients to balance the equation.
- Ensure the number of atoms of each element is the same on both sides.
Balancing Chemical Equations
- Count the number of atoms of each element on both sides of the equation.
- Add coefficients to balance the equation.
- Never change the subscripts in a chemical formula.
Examples of Chemical Equations
- 2H2 + O2 → 2H2O (Combustion of Hydrogen)
- CaO + H2O → Ca(OH)2 (Reaction of Calcium Oxide with Water)
Important Concepts
- Law of Conservation of Mass: Matter cannot be created or destroyed in a chemical reaction.
- Stoichiometry: The study of the quantitative relationships between reactants and products in a chemical reaction.
Chemical Reactions
- A chemical reaction is a process that involves the transformation of one or more substances into new substances.
Types of Chemical Reactions
- Synthesis reaction: two or more substances combine to form a new compound.
- Decomposition reaction: a single compound breaks down into two or more substances.
- Replacement reaction: one element replaces another element in a compound.
- Combustion reaction: a substance reacts with oxygen to produce heat and light.
Chemical Equations
- A chemical equation represents a chemical reaction using chemical formulas and symbols.
Parts of a Chemical Equation
- Reactants: substances that undergo a chemical change.
- Products: substances formed as a result of the chemical reaction.
- Arrow (→): indicates the direction of the reaction.
- Coefficients: whole numbers that indicate the relative amounts of reactants and products.
Writing Chemical Equations
- Write reactants on the left and products on the right.
- Use the arrow (→) to separate reactants and products.
- Use coefficients to balance the equation.
- Ensure the number of atoms of each element is the same on both sides.
Balancing Chemical Equations
- Count the number of atoms of each element on both sides of the equation.
- Add coefficients to balance the equation.
- Never change the subscripts in a chemical formula.
Examples of Chemical Equations
- Combustion of Hydrogen: 2H2 + O2 → 2H2O
- Reaction of Calcium Oxide with Water: CaO + H2O → Ca(OH)2
Important Concepts
- Law of Conservation of Mass: matter cannot be created or destroyed in a chemical reaction.
- Stoichiometry: the study of the quantitative relationships between reactants and products in a chemical reaction.
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Description
Learn about the different types of chemical reactions, including synthesis, decomposition, replacement, and combustion reactions.
