1 / 29

Chapter 6 Chemical Reactions and Quantities

Chapter 6 Chemical Reactions and Quantities. 6.1 Chemical Reactions. Chemical Change. In a chemical change , reacting substances form new substances with different compositions and properties a chemical reaction takes place. Evidence of Chemical Change. Chemical Reactions.

oharris
Download Presentation

Chapter 6 Chemical Reactions and Quantities

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. Chapter 6 Chemical Reactions and Quantities 6.1Chemical Reactions

  2. Chemical Change In a chemical change, • reacting substances form new substances with different compositions and properties • a chemical reaction takes place

  3. Evidence of Chemical Change

  4. Chemical Reactions In a chemical reaction, • a chemical change produces one or more new substances • there is a change in the composition of one or more substances

  5. Chemical Reactions (continued) In a chemical reaction, • old bonds are broken and new bonds formed • atoms in the reactants are rearranged to form one or more different substances

  6. Learning Check Identify the visible evidence of a chemical reaction in each of the following: 1) Methane gas in an outdoor heater burns with a blue flame. 2) Bleach removes stains from a shirt. 3) Bubbles of CO2 are released when baking soda is mixed with vinegar.

  7. Solution 1) Methane gas in an outdoor heater burns with a blue flame. Heat and a flame 2) Bleach removes stains from a shirt. Color change (color removed) 3) Bubbles of CO2 are released when baking soda is mixed with vinegar. Formation of gas (bubbles)

  8. Chemical Equations A chemical equation • gives the chemical formulas of the reactants on the left of the arrow and the products on the right

  9. Symbols Used in Equations Symbols used in chemical equations show • the states of the reactants • the states of the products • the reaction conditions

  10. Chemical Equations are Balanced In a balanced chemical reaction, • atoms are not lost or gained • the number of atoms in the reactants is equal to the number of atoms in the products

  11. A Balanced Chemical Equation In a balanced chemical equation, • there must be the same number of each type of atom on the reactant side and on the product side • numbers called coefficientsare used in front of one or more formulas. Al + S Al2S3 Not balanced 2Al + 3S Al2S3Balanced 2Al = 2Al 3S = 3S

  12. Learning Check State the number of atoms of each element on the reactant side and the product side for each of the following balanced equations: A. P4(s) + 6Br2(l) 4PBr3(g) B. 2Al(s) + Fe2O3(s) 2Fe(s) + Al2O3(s)

  13. Solution A. P4(s) + 6Br2(l) 4PBr3(g) 4 P 4 P 12 Br 12 Br B. 2Al(s) + Fe2O3(s) 2Fe(s) + Al2O3(s) 2 Al 2 Al 2 Fe 2 Fe 3 O 3 O

  14. Learning Check Determine if each equation is balanced or not. A. Na(s) + N2(g) Na3N(s) B. C2H4(g) + H2O(l) C2H5OH(l)

  15. Solution A. Na(s) + N2(g) Na3N(s) Not balanced 2N 1N 1Na 3Na B. C2H4(g) + H2O(l) C2H5OH(l) Balanced 2C 2C 6H 6H 1O 1O

  16. Equation for A Chemical Reaction

  17. Checking a Balanced Equation

  18. Guide to Balancing Equations

  19. Balancing Chemical Equations STEP 1 Write the equation with the correct formulas. N2(g) + H2(g) NH3(g) STEP 2 Determine if the equation is balanced. No, not all of the atoms are balanced. 2N 1N 2H 3H STEP 3 Balance with coefficients in front of formulas. Balance N N2(g) + H2(g) 2NH3(g)

  20. Balancing Chemical Equations (continued) STEP 3 (continued) Balance H N2(g) + 3H2(g) 2NH3(g) STEP 4 Check that atoms of each element are equal in reactants and products. 2N = 2N 6H = 6H

  21. Learning Check Check the balance of atoms in the following: Fe3O4(s) + 4H2(g) 3Fe(s) +4H2O(l) A. number of H atoms in products 1) 2 2) 4 3) 8 B. number of O atoms in reactants 1) 2 2) 4 3) 8 C. number of Fe atoms in reactants 1) 1 2) 3 3) 4

  22. Solution Fe3O4(s) + 4H2(g) 3Fe(s) +4H2O(l) A. number of H atoms in products 3) 8 (4H2O) B. number of O atoms in reactants 2) 4 (Fe3O4) C. number of Fe atoms in reactants 2) 3 (Fe3O4)

  23. Learning Check Balance each equation and list the coefficients in the balanced equation going from reactants to products. A. __Mg(s) + __N2(g) __Mg3N2(s) 1) 1, 3, 2 2) 3, 1, 2 3) 3, 1, 1 B. __Al(s) + __Cl2(g) __AlCl3(s) 1) 3, 3, 2 2) 1, 3, 1 3) 2, 3, 2

  24. Solution Balance each equation and list the coefficients in the balanced equation going from reactants to products. A. 3) 3, 1, 1 3Mg(s) + 1N2(g) 1Mg3N2(s) B. 3) 2, 3, 2 2Al(s) + 3Cl2(g) 2AlCl3(s)

  25. Equations with Polyatomic Ions

  26. Balancing with Polyatomic Ions STEP 1 Write the equation with the correct formulas. Na3PO4(aq) + MgCl2(aq) NaCl(aq) + Mg3(PO4)2(s) STEP 2 Determine if the equation is balanced. No, not all atoms are balanced. 3Na+ 1Na+ 1PO43 2PO43  1Mg2+ 3Mg2+ 2Cl 1Cl STEP 3 Balance with coefficients in front of formulas. Balance PO43as a unit. 2Na3PO4(aq) Mg3(PO4)2(s)

  27. Balancing with Polyatomic Ions (continued) STEP 3 (continued) Balance Mg 3MgCl2(aq) Mg3(PO4)2(s) Balance Na and Cl 3MgCl2(aq) + 2Na3PO4(aq) 6NaCl(aq) + Mg3(PO4)2(s) STEP 4 Check that atoms of each element are equal in reactants and products. 2PO43–= 2PO43– 3Mg2+ = 3Mg2+ 6Na+ = 6Na+ 6Cl= 6Cl

  28. Learning Check Balance and list the coefficients from reactants to products: A. __Fe2O3(s) + __C(s) __Fe(s) + __CO2(g) 1) 2, 3, 2,3 2) 2, 3, 4, 3 3) 1, 1, 2, 3 B. __Al(s) + __FeO(s) __Fe(s) + __Al2O3(s) 1) 2, 3, 3, 1 2) 2, 1, 1, 1 3) 3, 3, 3, 1 C. __Al(s) + __H2SO4(aq) __Al2(SO4)3(aq) + __H2(g) 1) 3, 2, 1, 22) 2, 3, 1, 3 3) 2, 3, 2, 3

  29. Solution A. 2) 2, 3, 4, 3 2Fe2O3(s)+ 3C(s) 4Fe(s) + 3CO2(g) B. 1) 2, 3, 3, 1 2Al(s) + 3FeO(s) 3Fe(s) + 1Al2O3(s) C. 2) 2, 3, 1, 3 2Al(s) + 3H2SO4(aq) 1Al2(SO4)3(aq) + 3H2(g)

More Related