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What is a precipitate?
What is a precipitate?
An insoluble compound that comes out of the solution.
Describe the characteristics of the five types of chemical reactions.
Describe the characteristics of the five types of chemical reactions.
1.) Synthesis: 2 or more reactants combine to make 1 product. 2.) Decomposition: When 1 reactant breaks down into 2 or more products. 3.) Combustion: When something is burned, with oxygen (O2) as a reactant and carbon dioxide (CO2) and water (H2O) as products. 4.) Single Replacement: One element replaces a similar element in a compound. 5.) Double Replacement: Two ionic compound reactants switch ions, forming two new ionic compound products, usually resulting in a precipitate.
Classify the reaction: AlBr3 + K2SO4 = KBr + Al2(SO4)3.
Classify the reaction: AlBr3 + K2SO4 = KBr + Al2(SO4)3.
Double Replacement
Classify the reaction: Al + O2 = Al2O3.
Classify the reaction: Al + O2 = Al2O3.
Classify the reaction: LiCl + Br2 = LiBr + Cl2.
Classify the reaction: LiCl + Br2 = LiBr + Cl2.
Classify the reaction: NF3 = N2 + F2.
Classify the reaction: NF3 = N2 + F2.
Classify the reaction: C4H10 + O2 = CO2 + H2O.
Classify the reaction: C4H10 + O2 = CO2 + H2O.
Classify the reaction: Pb(OH)2 + HCl = H2O + PbCl2.
Classify the reaction: Pb(OH)2 + HCl = H2O + PbCl2.
Write out the balanced chemical reaction for the reaction of solid sulfur with solid iron to form solid iron (III) sulfide.
Write out the balanced chemical reaction for the reaction of solid sulfur with solid iron to form solid iron (III) sulfide.
Write out the balanced chemical reaction for the reaction of hydrogen gas and iron (III) oxide to form water and iron powder.
Write out the balanced chemical reaction for the reaction of hydrogen gas and iron (III) oxide to form water and iron powder.
Write out the balanced chemical reaction for the combustion of C3H8.
Write out the balanced chemical reaction for the combustion of C3H8.
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Study Notes
Precipitation
- Precipitate refers to an insoluble compound that emerges from a solution.
Types of Chemical Reactions
- Synthesis: Involves two or more reactants combining to form a single product.
- Decomposition: A single reactant breaks down into two or more products.
- Combustion: A reaction where a substance is burned, always involving oxygen (O2) as a reactant and producing carbon dioxide (CO2) and water (H2O) as products.
- Single Replacement: One element in a compound is replaced by a similar element from another compound.
- Double Replacement: Two ionic compounds react and exchange ions, typically resulting in the formation of a precipitate.
Reaction Classifications
- Double Replacement: AlBr3 + K2SO4 = KBr + Al2(SO4)3.
- Synthesis: Al + O2 = Al2O3.
- Single Replacement: LiCl + Br2 = LiBr + Cl2.
- Decomposition: NF3 = N2 + F2.
- Combustion: C4H10 + O2 = CO2 + H2O.
- Double Replacement: Pb(OH)2 + HCl = H2O + PbCl2.
Reaction Balancing and Classification
- Synthesis Reaction: 3S + 2Fe = Fe2S3 (Solid sulfur reacts with solid iron to form solid iron (III) sulfide).
- Single Replacement Reaction: 3H2 + Fe2O3 = 3H2O + 2Fe (Hydrogen gas reacts with iron (III) oxide to produce water and iron powder).
- Combustion Reaction: C3H8 + 5O2 = 3CO2 + 4H2O (C3H8 is burned).
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