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Questions and Answers
Which of the following is an example of a combination reaction?
Which of the following is an example of a combination reaction?
In a balanced chemical equation, the number of atoms of each element on the reactant side must be less than the number of atoms of the same element on the product side.
In a balanced chemical equation, the number of atoms of each element on the reactant side must be less than the number of atoms of the same element on the product side.
False (B)
In the reaction 2AgCl + sunlight → 2Ag(s) + Cl2(g), what color change is observed?
In the reaction 2AgCl + sunlight → 2Ag(s) + Cl2(g), what color change is observed?
What is the term for a reaction that releases heat?
What is the term for a reaction that releases heat?
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The decomposition of water into hydrogen and oxygen via electric current is known as ______ decomposition.
The decomposition of water into hydrogen and oxygen via electric current is known as ______ decomposition.
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In a displacement reaction, a less reactive element replaces a more reactive element from its compound.
In a displacement reaction, a less reactive element replaces a more reactive element from its compound.
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Match the following terms with their descriptions:
Match the following terms with their descriptions:
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What is the name given to a reaction where ions are exchanged between reactants?
What is the name given to a reaction where ions are exchanged between reactants?
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The reaction CH4(g) + O2(g) → CO2(g) + H2O(g) + Heat is a example of a(n) _______ reaction?
The reaction CH4(g) + O2(g) → CO2(g) + H2O(g) + Heat is a example of a(n) _______ reaction?
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Match the following terms with their correct definitions:
Match the following terms with their correct definitions:
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Study Notes
Chemical Reactions and Equations
- Chemical reaction: A process where new substances are formed from existing ones
- Chemical equations: Symbolic representations of chemical reactions
- Balanced chemical equations: Equations with equal numbers of atoms of each element on both sides of the equation
- Conservation of mass: The principle stating that mass is neither created nor destroyed in a chemical reaction
- Balancing chemical reactions: A process requiring an equal number of atoms of each element on both sides
Types of Chemical Reactions
Combination Reactions
- Two or more reactants combine to form a single product.
- Examples include magnesium reacting with oxygen to form magnesium oxide.
Decomposition Reactions
- A single reactant breaks down into two or more products.
- This can occur through heat (thermal decomposition), electricity (electrolysis), or light (photochemical decomposition).
- Examples include calcium carbonate decomposing into calcium oxide and carbon dioxide.
Displacement Reactions
- More reactive elements replace less reactive elements in a compound
- Reactivity series of elements determines which element will be displaced.
- Examples include iron reacting with copper sulfate to form iron sulfate and copper
Double Displacement Reactions
- Exchange of ions between reacting substances.
- Resulting products often include a precipitate (solid), gas, or water.
- Examples include mixing sodium sulfate and barium chloride solutions to form barium sulfate precipitate.
Heat in Reactions
- Exothermic reactions: Release heat
- Endothermic reactions: Absorb heat
Redox Reactions
- Reactions involving simultaneous oxidation and reduction
- Oxidation: Loss of electrons, gain of oxygen, loss of hydrogen
- Reduction: Gain of electrons, loss of oxygen, gain of hydrogen
Corrosion
- Deterioration of metals due to interaction with the environment
- Rusting of iron is a common example
Rancidity
- Spoilage of food containing fats or oils due to oxidation
- Prevention through refrigeration and other methods
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Description
Test your knowledge on chemical reactions and equations, including types of reactions such as combination and decomposition. Explore key concepts like balancing equations and the conservation of mass. This quiz covers fundamental principles that are essential for understanding chemistry.
