Chapter 8.1 : Describing Chemical Reactions
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The document describes chemical equations and reactions, including: - Three observations that indicate a chemical reaction has occurred and three requirements for a correctly written chemical equation. - Examples of word and formula equations and how to balance a chemical equation to satisfy the law of conservation of mass. - Additional symbols used in chemical equations and the significance of coefficients in a balanced chemical equation.
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Chapter 7.1 : Chemical Names and Formulas
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This document discusses chemical equations and reactions. It defines a chemical reaction as a process where one or more substances are changed into one or more different substances. A chemical equation represents the identities and relative amounts of reactants and products in a chemical reaction. Writing a proper chemical equation involves first writing a word equation, then a formula equation, and finally balancing the equation so the same number and type of atoms are on both sides. Common techniques for writing and balancing chemical equations are explained.
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The document discusses chemical reactions and equations. It provides information on:
- Writing balanced chemical equations to represent reactions
- Indications that a reaction occurred like heat/gas production
- Characteristics of chemical equations like conservation of mass
- Examples of balancing equations and writing equations for reactions
Balancing Equations and Reactions
Chemical equations are used to represent chemical reactions. They show the formulas of the reactants and products, with coefficients indicating relative amounts. A word equation also describes the reaction using names. Various symbols are used to indicate state, catalysts or conditions. For the equation to be correct, it must be balanced to satisfy the law of conservation of matter, with the same number and type of atoms on each side. Balancing ensures the amounts of elements are equal before and after reaction.
Chemistry reaction.pdf
1) Chemical equations represent chemical reactions through formulas showing reactants and products. They must be balanced to satisfy the law of conservation of mass.
2) Types of chemical reactions include synthesis, decomposition, single replacement, double replacement, combustion and more. Balancing equations ensures the same number and types of atoms are on each side.
3) Additional symbols specify physical states like (s) solid, (l) liquid, (g) gas. Solubility rules predict if ionic compounds will dissolve or precipitate out of solution.
Science 10th Class
This document provides information on stoichiometry, which involves using mole ratios from balanced chemical equations to calculate mass relationships between substances in a chemical reaction. It outlines the steps to solve stoichiometry problems, which include writing a balanced equation, identifying known and unknown quantities, setting up mole ratio conversion factors between moles of reactants and products, and checking the answer. Key concepts discussed include the mole ratio from coefficients in a balanced equation, molar mass to convert between moles and grams, and the molar volume used to calculate liters of gas at standard temperature and pressure.
Chpt 9 chemical equations ver2
Chemical equations show:
1. The reactants and products of a chemical reaction.
2. The physical states of reactants and products using standard abbreviations like (s) for solid and (g) for gas.
3. Additional information like the progress of the reaction using arrows, the presence of a catalyst, or added heat.
Chemical equations & reactions
The document discusses chemical equations and reactions. It defines key terms like reactants, products, and coefficients. It explains how to write and balance chemical equations. It also describes different types of chemical reactions like synthesis, decomposition, and single/double replacement reactions. Guidelines are provided for predicting products and writing balanced equations.
Chemunit8presentation 120129161435-phpapp02
This document provides information about chemical reactions and equations. It discusses the main types of chemical reactions including synthesis, combustion, decomposition, and replacement reactions. It also explains how chemical reactions are represented by balanced chemical equations, which show the relative amounts of reactants and products. Double replacement reactions that occur in aqueous solutions are also covered, and can produce precipitates, water, or gases.
CHEMICAL EQUATIONS AND REACTIONS
1. Chemical reactions involve chemical changes that result in the formation of new substances.
2. Chemical equations are used to represent chemical reactions, with reactants on the left side of the arrow and products on the right. These equations must be balanced and follow the law of conservation of mass.
3. There are several types of chemical reactions including combination, decomposition, displacement, and oxidation-reduction. Combination reactions involve elements or compounds reacting to form a single product, while decomposition reactions involve a single reactant breaking down into simpler products.
Mirakle puhan sc.
1. Chemical reactions can be represented through word equations, chemical equations, and balanced chemical equations.
2. There are several types of chemical reactions including combination, decomposition, displacement, and oxidation-reduction.
3. Word equations show the reactants and products of a chemical reaction using chemical names. Chemical equations use chemical formulas and are balanced to satisfy the law of conservation of mass.
Chapter 8
The document provides information about chemical reactions, including defining reactants and products, describing types of chemical reactions like synthesis, decomposition, double displacement, displacement and combustion reactions. It also discusses how to write and balance chemical equations.
Chemical equations and reactions
1. Chemical reactions involve chemical changes where reactants are converted into products. Signs of a chemical reaction include changes in color, gas evolution, temperature changes, and state changes.
2. A word equation represents the reactants and products of a chemical reaction using chemical names. A balanced chemical equation uses formulas to represent the reactants on the left and products on the right, separated by an arrow.
3. There are several types of chemical reactions including combination, decomposition, displacement, and redox reactions. Combination reactions involve reactants combining to form compounds while decomposition reactions involve splitting compounds into simpler substances.
Chapter 11
This document describes chemical reactions and equations. It discusses:
1. The components of chemical equations including reactants and products.
2. The different types of chemical equations including word equations, skeleton equations, and chemical equations.
3. How to balance chemical equations by ensuring equal numbers of each type of atom on both sides of the reaction arrow.
4. The five major types of chemical reactions - combination, decomposition, single replacement, double replacement, and combustion.
5. How to predict whether a precipitation reaction will occur based on solubility rules for ionic compounds.
Chemical Reactions
A chemical reaction involves the transformation of reactants into different products through rearrangement of atoms. Chemical reactions conserve mass as atoms are not destroyed or created, but instead are reorganized into new substances. Balancing chemical equations ensures the same number and type of atoms are on both sides of the reaction.
5- Chemical Reactions.pptx
The document discusses chemical reactions and stoichiometry. It defines chemical reactions as processes where substances are changed into new substances. Reactants are the original substances, and products are the new substances formed. The document covers types of chemical reactions like combustion and replacement reactions. It also discusses balancing chemical equations, mole ratios, and using mole-mole calculations to solve stoichiometry problems involving masses of reactants and products. An example uses a balanced equation to determine the mass of CO2 produced given the mass of CH4 consumed.
Chem unit 8 presentation
Polyatomic ions stay intact in aqueous solutions because they are held together by strong covalent bonds between their constituent atoms. When ionic compounds dissolve in water, the ions separate but polyatomic ions remain intact units because the covalent bonds within them are not broken by the dissociation process.
Chemical reactions and equations Class 10
Chemical, Reactions and Equations Class 10 Chemistry full explanation withe examples as well as step by step explainations
Balancing Equations
A chemical equation represents a chemical reaction using formulas to show the reactants and products. It uses coefficients to indicate the ratio in which substances react or are produced, and parentheses to show the state of each substance. A chemical reaction conserves mass according to the law of conservation of mass. There are four main types of chemical reactions: synthesis, decomposition, single replacement, and double replacement.
Chem unit 8 presentation
This document discusses chemical reactions and how they are represented. It covers the following key points:
1. Chemical reactions are represented by balanced chemical equations that show the reactants and products. There are four main types of reactions: synthesis, combustion, decomposition, and replacement.
2. Double replacement reactions occur between ionic compounds in aqueous solution and often produce a precipitate, water, or a gas.
3. Chemical equations must be balanced to obey the law of conservation of mass. This involves determining coefficients for the reactants and products so that the number of atoms of each element is equal on both sides of the reaction.
Chemical Reaction
This presentation is prepare by Gunjan Bhandary studying in class 9 of Baylor International Academy located in Banepa, Nepal
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Chapter 8.1 : Describing Chemical Reactions
- 1. Chemical equations and reactions Chapter 8.1
- 2. Objectives: List three observations that suggest that a chemical reaction has taken place. List three requirements for a correctly written chemical equation. Write a word equation and a formula equation for a given chemical reaction. Balance a formula equation by inspection.
- 4. Defined as represents, with symbols and formulas, the identities and relative amounts of the reactants and products in a chemical reaction.
- 5. Example: this chemical equation shows the reactant ammonium dichromate yields the products nitrogen, chromium(III) oxide, and water(NH4)2Cr2O7(s) N2(g) + Cr2O3(s) + 4H2O(g)
- 6. Indications of Chemical Reactions Evolution of heat and light Production of gas Formation of a precipitate Color change Chemistry comes alive!
- 8. Coefficients are added where necessary
- 9. Specifies relative number of moles of that substanceEx: Hydrogen gas reacts with oxygen gas to yield water H2 + O2 H2O 2 2
- 12. formula equation - 2ndstep in writing chemical equation
- 13. Represents the reactants and products of a chemical reaction by their symbol
- 14. Example:
- 15. (g) represents that it is in gaseous stateCH4 (g) + O2 (g) CO2 (g) + H2O (g)
- 16. balance the equation– last step in writing a chemical equation Satisfy law of conservation of mass by inserting coefficients # of atoms of reactant must = # of atoms of products 2 2 Reactant Product Step 1: Type & number C C 1 1 Step 3: When reactants = products its balanced H H 4 2 4 Step 2: Add coefficients till reactants = products O O 2 3 4 4 CH4 (g) + O2 (g) CO2 (g) + H2O (g)
- 17. Additional symbols used in chemical reactions Examples: Yields Reversible reactions (s) or solid state (g) or gaseous state (l) liquid state (aq) aqueous (dissolved in water) reactants are heated 2 atm Pressure 0⁰ C Temperature MnO2 Catalyst 3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g) 2HgO(s) 2Hg(l) + O2(g) C2H2(s) + H2(g) pressure C2H6(g) Pt
- 19. Reverse reaction for a chemical reaction has the same relative amounts of substances as the forward reaction Balancing Chemical Equations Identify the names of the reactants and the products, and write a word equation. water hydrogen + oxygen Write a formula equation by substituting correct formulas for the names of the reactants and the products. H2O(g) H2(g) + O2(g)
- 21. First balance the atoms of elements that are combined and that appear only once on each side of the equation
- 22. Balance polyatomic ions that appear on both sides of the equation as single units.
- 23. Balance H atoms and O atoms after atoms of all other elements have been balancedH2O(g) H2(g) + O2(g) 2 2 Product Reactant H H 2 2 4 4 O O 1 2 2 Count atoms to be sure that the equation is balanced.
- 25. Step 2: convert to formula equation Step 3: add all symbols 2 Na2O + H2O NaOH (s) (l) (aq) Step 4: balance Reactant Product Na 2 1 Na 2 2 H 1 2 H 2 O 1 2 O Practice 2 Translate the following chemical reaction PbCl2(aq) + Na2CrO4(aq) PbCrO4(s) + 2 NaCl(aq) Aqueous lead(II) chloride reacts with aqueous sodium chromate to produce a precipitate of lead(II) chromate and aqueous sodium chloride.
- 27. Practice 3 The reaction of zinc with aqueous hydrochloric acid produces a solution of zinc chloride and hydrogen gas. Write the balanced chemical equation for the reaction. zinc + hydrochloric acid zinc chloride + hydrogen Zn(s) + HCl(aq) ZnCl2(aq) + H2(g) 2 Reactant Product Zn 1 1 Zn 1 H 2 2 H 2 1 Cl 2 Cl
- 28. Practice 4 Solid aluminum carbide, Al4C3, reacts with water to produce methane gas and solid aluminum hydroxide. Write a balanced chemical equation for this reaction. Aluminum carbide + water + aluminum hydroxide methane 3 4 Al4C3(s) + H2O(l) + Al(OH)3(s) CH4(g) 12 Reactant Product 4 4 1 Al Al 3 3 1 C C 24 24 7 15 2 H H 12 1 3 12 O O
- 29. Practice 5 Aluminum sulfate and calcium hydroxide are used in a water-purification process. When added to water, they dissolve and react to produce two insoluble products, aluminum hydroxide and calcium sulfate. These products settle out, taking suspended solid impurities with them. Write a balanced chemical equation for the reaction. Aluminum sulfate + Calcium hydroxide + calcium sulfate aluminum hydroxide Al2(SO4)3 (aq) + 2 3 3 Ca(OH)2(aq) + CaSO4(s) Al(OH)3(s) Reactant Product 2 1 2 Al Al 3 1 3 SO4 SO4 3 3 1 1 Ca Ca 6 2 3 6 OH OH