<ul><li>Balance the following chemical equations by adding coefficients in front of the compounds. </li></ul><ul><li>Examp...
<ul><li>Balance the following chemical equations by adding coefficients in front of the compounds. </li></ul><ul><li>Examp...
<ul><ul><ul><li>A balanced chemical equation provides the same kind of quantitative information that a recipe does. </li><...
<ul><ul><li>Mass and atoms are conserved in every chemical reaction. </li></ul></ul><ul><ul><li>Mass of reactants = mass o...
<ul><ul><ul><li>A balanced chemical equation can be interpreted in terms of different quantities.  </li></ul></ul></ul><ul...
N 2 (g)  +  3H 2 (g)     2NH 3 (g)  2 N  +  6 H  =  2 N  +  6H Atoms are conserved!!
Coefficients tell us the RATIO of molecules  N 2 (g)  +  3H 2 (g)     2NH 3 (g)
Coefficients tell us the RATIO of molecules  one N 2   +  three H 2      two NH 3 molecule  molecules  molecules   N 2 (g...
Coefficients tell us the RATIO of moles  N 2 (g)  +  3H 2 (g)     2NH 3 (g)
one mole +  three moles    two moles N 2   H 2   NH 3   Coefficients tell us the RATIO of moles  N 2 (g)  +  3H 2 (g)   ...
Find the molar mass of each compound & multiply by the coefficient   N 2 (g)  +  3H 2 (g)     2NH 3 (g)
28g   +  3 x 2g     2 x 17g N 2 (g)  +  3H 2 (g)     2NH 3 (g)  Find the molar mass of each compound & multiply by the c...
28g   +  3 x 2g     2 x 17g Why do you multiply the molar mass by three? N 2 (g)  +  3H 2 (g)     2NH 3 (g)  Find the mo...
28g   +  3 x 2g     2 x 17g 28g  +  6g     34g  N 2 (g)  +  3H 2 (g)     2NH 3 (g)  Find the molar mass of each compoun...
34g = 34g Mass is conserved! 28g   +  3 x 2g     2 x 17g 28g  +  6g     34g  N 2 (g)  +  3H 2 (g)     2NH 3 (g)  Find t...
N 2 (g)  +  3H 2 (g)     2NH 3 (g)  At STP, one mole of  gas occupies 22.4 liters.
22.4L N 2  +  3  22.4L H 2    2  22.4L   NH 3 N 2 (g)  +  3H 2 (g)     2NH 3 (g)  At STP, one mole of  gas occupies 22...
N 2 (g)  +  3H 2 (g)     2NH 3 (g)  At STP, one mole of  gas occupies 22.4 liters. 22.4L N 2  +  3  22.4L H 2    2  22...
N 2 (g)  +  3H 2 (g)     2NH 3 (g)  At STP, one mole of  gas occupies 22.4 liters. 22.4L N 2  +  67.2L H 2     44.8L   N...
<ul><ul><ul><li>Chemists use  stoichiometry  and  mole ratios  to calculate how much reactant is needed or how much produc...
<ul><ul><ul><li>The first step in stoichiometry is to get a balanced equation. </li></ul></ul></ul>
<ul><ul><ul><li>The first step in stoichiometry is to get a balanced equation. </li></ul></ul></ul><ul><ul><ul><li>H 2  + ...
<ul><ul><ul><li>The first step in stoichiometry is to get a balanced equation. </li></ul></ul></ul><ul><ul><ul><li>H 2  + ...
<ul><ul><ul><li>The first step in stoichiometry is to get a balanced equation. </li></ul></ul></ul><ul><ul><ul><li>H 2  + ...
<ul><ul><ul><li>The first step in stoichiometry is to get a balanced equation. </li></ul></ul></ul><ul><ul><ul><li>H 2  + ...
<ul><ul><ul><li>2H 2  + O 2     2H 2 O </li></ul></ul></ul><ul><ul><ul><li>How many moles of O 2  are needed to completel...
<ul><ul><ul><li>2H 2  + O 2     2H 2 O </li></ul></ul></ul><ul><ul><ul><li>How many moles of O 2  are needed to completel...
Conceptual Problem 12.1
Conceptual Problem 12.1
Conceptual Problem 12.1
<ul><ul><li>Production of iron metal from iron ore–  </li></ul></ul><ul><ul><li>Fe 2 O 3 •H 2 O( s ) + 3CO( g )    2Fe( s...
<ul><ul><li>What is conserved in the following reaction?  </li></ul></ul><ul><ul><ul><ul><li>H 2 ( g ) + Cl 2 ( g )    2H...
Upcoming SlideShare
Loading in …5
×

Lecture 12.1- Interpreting Balanced Equations

6,896 views

Published on

Section 12.1 Lecture for Honors & Prep Chemistry

Published in: Education, Technology
0 Comments
1 Like
Statistics
Notes
  • Be the first to comment

No Downloads
Views
Total views
6,896
On SlideShare
0
From Embeds
0
Number of Embeds
20
Actions
Shares
0
Downloads
51
Comments
0
Likes
1
Embeds 0
No embeds

No notes for slide
  • A cookie recipe tells you the number of cookies that you can expect to make from the listed amounts of ingredients. Using Models How can you express a cookie recipe as a balanced equation?
  • The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH 3 could be made from 5 molecules of N 2 and 15 molecules of H 2 ?
  • The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH 3 could be made from 5 molecules of N 2 and 15 molecules of H 2 ?
  • The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH 3 could be made from 5 molecules of N 2 and 15 molecules of H 2 ?
  • The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH 3 could be made from 5 molecules of N 2 and 15 molecules of H 2 ?
  • The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH 3 could be made from 5 molecules of N 2 and 15 molecules of H 2 ?
  • The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH 3 could be made from 5 molecules of N 2 and 15 molecules of H 2 ?
  • The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH 3 could be made from 5 molecules of N 2 and 15 molecules of H 2 ?
  • The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH 3 could be made from 5 molecules of N 2 and 15 molecules of H 2 ?
  • The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH 3 could be made from 5 molecules of N 2 and 15 molecules of H 2 ?
  • The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH 3 could be made from 5 molecules of N 2 and 15 molecules of H 2 ?
  • The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH 3 could be made from 5 molecules of N 2 and 15 molecules of H 2 ?
  • The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH 3 could be made from 5 molecules of N 2 and 15 molecules of H 2 ?
  • The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH 3 could be made from 5 molecules of N 2 and 15 molecules of H 2 ?
  • The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH 3 could be made from 5 molecules of N 2 and 15 molecules of H 2 ?
  • Lecture 12.1- Interpreting Balanced Equations

    1. 1. <ul><li>Balance the following chemical equations by adding coefficients in front of the compounds. </li></ul><ul><li>Example- 2 H 2 + O 2  2 H 2 O </li></ul><ul><li>1 . MgCl 2 + AgNO 3  AgCl + Mg(NO 3 ) 2 </li></ul><ul><li>2. C 3 H 8 + O 2  CO 2 + H 2 O </li></ul><ul><li>3. Al + AgNO 3  Ag + Al(NO 3 ) 3 </li></ul><ul><li>4. C 12 H 22 O 11  C + H 2 O </li></ul><ul><li>An unbalanced equation is mathematically useless! </li></ul>Bellwork
    2. 2. <ul><li>Balance the following chemical equations by adding coefficients in front of the compounds. </li></ul><ul><li>Example- 2 H 2 + O 2  2 H 2 O </li></ul><ul><li>1 . MgCl 2 + AgNO 3  AgCl + Mg(NO 3 ) 2 </li></ul><ul><li>2. C 3 H 8 + O 2  CO 2 + H 2 O </li></ul><ul><li>3. Al + AgNO 3  Ag + Al(NO 3 ) 3 </li></ul><ul><li>4. C 12 H 22 O 11  C + H 2 O </li></ul><ul><li>An unbalanced equation is mathematically useless! </li></ul>Bellwork NEVER change subscripts
    3. 3. <ul><ul><ul><li>A balanced chemical equation provides the same kind of quantitative information that a recipe does. </li></ul></ul></ul>
    4. 4. <ul><ul><li>Mass and atoms are conserved in every chemical reaction. </li></ul></ul><ul><ul><li>Mass of reactants = mass of products </li></ul></ul><ul><ul><li>Number and type of atoms in reactants = number & type atoms in products </li></ul></ul>
    5. 5. <ul><ul><ul><li>A balanced chemical equation can be interpreted in terms of different quantities. </li></ul></ul></ul><ul><ul><ul><li>numbers of atoms </li></ul></ul></ul><ul><ul><ul><li>Molecules </li></ul></ul></ul><ul><ul><ul><li>Moles </li></ul></ul></ul><ul><ul><ul><li>Mass </li></ul></ul></ul><ul><ul><ul><li>volume. </li></ul></ul></ul><ul><ul><ul><li>N 2 (g) + 3H 2 (g)  2NH 3 (g) </li></ul></ul></ul>
    6. 6. N 2 (g) + 3H 2 (g)  2NH 3 (g) 2 N + 6 H = 2 N + 6H Atoms are conserved!!
    7. 7. Coefficients tell us the RATIO of molecules N 2 (g) + 3H 2 (g)  2NH 3 (g)
    8. 8. Coefficients tell us the RATIO of molecules one N 2 + three H 2  two NH 3 molecule molecules molecules N 2 (g) + 3H 2 (g)  2NH 3 (g)
    9. 9. Coefficients tell us the RATIO of moles N 2 (g) + 3H 2 (g)  2NH 3 (g)
    10. 10. one mole + three moles  two moles N 2 H 2 NH 3 Coefficients tell us the RATIO of moles N 2 (g) + 3H 2 (g)  2NH 3 (g)
    11. 11. Find the molar mass of each compound & multiply by the coefficient N 2 (g) + 3H 2 (g)  2NH 3 (g)
    12. 12. 28g + 3 x 2g  2 x 17g N 2 (g) + 3H 2 (g)  2NH 3 (g) Find the molar mass of each compound & multiply by the coefficient
    13. 13. 28g + 3 x 2g  2 x 17g Why do you multiply the molar mass by three? N 2 (g) + 3H 2 (g)  2NH 3 (g) Find the molar mass of each compound & multiply by the coefficient
    14. 14. 28g + 3 x 2g  2 x 17g 28g + 6g  34g N 2 (g) + 3H 2 (g)  2NH 3 (g) Find the molar mass of each compound & multiply by the coefficient
    15. 15. 34g = 34g Mass is conserved! 28g + 3 x 2g  2 x 17g 28g + 6g  34g N 2 (g) + 3H 2 (g)  2NH 3 (g) Find the molar mass of each compound & multiply by the coefficient
    16. 16. N 2 (g) + 3H 2 (g)  2NH 3 (g) At STP, one mole of gas occupies 22.4 liters.
    17. 17. 22.4L N 2 + 3  22.4L H 2  2  22.4L NH 3 N 2 (g) + 3H 2 (g)  2NH 3 (g) At STP, one mole of gas occupies 22.4 liters.
    18. 18. N 2 (g) + 3H 2 (g)  2NH 3 (g) At STP, one mole of gas occupies 22.4 liters. 22.4L N 2 + 3  22.4L H 2  2  22.4L NH 3 22.4L 22.4L 22.4L 22.4L 22.4L 22.4L
    19. 19. N 2 (g) + 3H 2 (g)  2NH 3 (g) At STP, one mole of gas occupies 22.4 liters. 22.4L N 2 + 67.2L H 2  44.8L NH 3 22.4L N 2 + 3  22.4L H 2  2  22.4L NH 3 22.4L 22.4L 22.4L 22.4L 22.4L 22.4L
    20. 20. <ul><ul><ul><li>Chemists use stoichiometry and mole ratios to calculate how much reactant is needed or how much product will be formed. </li></ul></ul></ul>
    21. 21. <ul><ul><ul><li>The first step in stoichiometry is to get a balanced equation. </li></ul></ul></ul>
    22. 22. <ul><ul><ul><li>The first step in stoichiometry is to get a balanced equation. </li></ul></ul></ul><ul><ul><ul><li>H 2 + O 2  H 2 O unbalanced (why?) </li></ul></ul></ul>
    23. 23. <ul><ul><ul><li>The first step in stoichiometry is to get a balanced equation. </li></ul></ul></ul><ul><ul><ul><li>H 2 + O 2  H 2 O unbalanced (why?) </li></ul></ul></ul><ul><ul><ul><li>2H 2 + O 2  2H 2 O balanced </li></ul></ul></ul>
    24. 24. <ul><ul><ul><li>The first step in stoichiometry is to get a balanced equation. </li></ul></ul></ul><ul><ul><ul><li>H 2 + O 2  H 2 O unbalanced (why?) </li></ul></ul></ul><ul><ul><ul><li>2H 2 + O 2  2H 2 O balanced </li></ul></ul></ul><ul><ul><ul><li>simple stoichiometry- How many moles of hydrogen gas are needed to make two moles of water? </li></ul></ul></ul>
    25. 25. <ul><ul><ul><li>The first step in stoichiometry is to get a balanced equation. </li></ul></ul></ul><ul><ul><ul><li>H 2 + O 2  H 2 O unbalanced (why?) </li></ul></ul></ul><ul><ul><ul><li>2H 2 + O 2  2H 2 O balanced </li></ul></ul></ul><ul><ul><ul><li>simple stoichiometry- How many moles of hydrogen gas are needed to make two moles of water? </li></ul></ul></ul>2 moles of H 2 ( g )
    26. 26. <ul><ul><ul><li>2H 2 + O 2  2H 2 O </li></ul></ul></ul><ul><ul><ul><li>How many moles of O 2 are needed to completely react with 4 moles of H 2 ? </li></ul></ul></ul>
    27. 27. <ul><ul><ul><li>2H 2 + O 2  2H 2 O </li></ul></ul></ul><ul><ul><ul><li>How many moles of O 2 are needed to completely react with 4 moles of H 2 ? </li></ul></ul></ul>2 moles of O 2 ( g )
    28. 28. Conceptual Problem 12.1
    29. 29. Conceptual Problem 12.1
    30. 30. Conceptual Problem 12.1
    31. 31. <ul><ul><li>Production of iron metal from iron ore– </li></ul></ul><ul><ul><li>Fe 2 O 3 •H 2 O( s ) + 3CO( g )  2Fe( s ) + 3CO 2 ( g ) + H 2 O( g ) </li></ul></ul><ul><ul><li>In this equation, the volume of gas at STP that reacts and the volume of gas at STP produced will be </li></ul></ul><ul><ul><ul><li>3 L and 4 L. </li></ul></ul></ul><ul><ul><ul><li>67.2 L and 89.6 L. </li></ul></ul></ul><ul><ul><ul><li>67.2 L and 67.2 L </li></ul></ul></ul><ul><ul><ul><li>3 L and 3 L </li></ul></ul></ul>
    32. 32. <ul><ul><li>What is conserved in the following reaction? </li></ul></ul><ul><ul><ul><ul><li>H 2 ( g ) + Cl 2 ( g )  2HCl( g ) </li></ul></ul></ul></ul><ul><ul><ul><li>only mass </li></ul></ul></ul><ul><ul><ul><li>only mass and number of moles </li></ul></ul></ul><ul><ul><ul><li>only mass, number of moles, and number of molecules </li></ul></ul></ul><ul><ul><ul><li>mass, number of moles, number of molecules, and volume </li></ul></ul></ul>

    ×