Bellwork-  Simple Stoich <ul><li>H 2 O 2 (aq)     H 2 O (l)  +  O 2 (g) </li></ul><ul><li>1. Balance the equation </li></...
<ul><ul><li>If given a quantity for one compound in a balanced equation you can calculate quantities for all of the others...
<ul><ul><ul><li>A  mole ratio  is a conversion factor made with the coefficients of a balanced chemical equation. </li></u...
<ul><ul><ul><li>A  mole ratio  is a conversion factor made with the coefficients of a balanced chemical equation. </li></u...
<ul><ul><li>N 2 ( g )  +  3H 2 ( g )     2NH 3 ( g ) </li></ul></ul>Use a mole ratio to convert between two different com...
<ul><li>STOICHIOMETRY </li></ul><ul><li>You need a balanced equation. </li></ul><ul><li>Convert the given quantity to mole...
for Sample Problem 12.2
<ul><ul><ul><li>For Stoichiometry–  </li></ul></ul></ul><ul><ul><ul><li>You ALWAYS use moles!! </li></ul></ul></ul><ul><ul...
<ul><ul><li>1. How many moles of water are produced when 2.5 mol of O 2  react according to the following equation? </li><...
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Lecture 12.2a- Mol-Mol Stoich

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Section 12.2a lecture for Honors & Prep Chemistry

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  • Manufacturing plants produce ammonia by combining nitrogen with hydrogen. Ammonia is used in cleaning products, fertilizers, and in the manufacture of other chemicals.
  • Lecture 12.2a- Mol-Mol Stoich

    1. 1. Bellwork- Simple Stoich <ul><li>H 2 O 2 (aq)  H 2 O (l) + O 2 (g) </li></ul><ul><li>1. Balance the equation </li></ul><ul><li>2. How many moles of H 2 O 2 must decompose in order to get 2 moles of O 2 (g)? </li></ul><ul><li>3. How many liters of O 2 (g) are formed from the decomposition of 2 moles of H 2 O 2 at STP? </li></ul><ul><li>4. Which are conserved in this reaction- Atoms, molecules, volume, moles, mass? </li></ul>
    2. 2. <ul><ul><li>If given a quantity for one compound in a balanced equation you can calculate quantities for all of the others using stoichiometry . </li></ul></ul><ul><ul><li>Example- 2 moles of N 2 requires ____moles of H 2 and will produce ____moles of NH 3. </li></ul></ul><ul><ul><li>N 2 ( g ) + 3H 2 ( g )  2NH 3 ( g ) Reactant #1 Reactant #2 Product </li></ul></ul>6 4
    3. 3. <ul><ul><ul><li>A mole ratio is a conversion factor made with the coefficients of a balanced chemical equation. </li></ul></ul></ul><ul><ul><li>N 2 ( g ) + 3H 2 ( g )  2NH 3 ( g ) </li></ul></ul>
    4. 4. <ul><ul><ul><li>A mole ratio is a conversion factor made with the coefficients of a balanced chemical equation. </li></ul></ul></ul><ul><ul><li>N 2 ( g ) + 3H 2 ( g )  2NH 3 ( g ) </li></ul></ul><ul><ul><li>Some mole ratios: </li></ul></ul><ul><ul><li>1 mole N 2 3 moles H 2 1 mole N 2 </li></ul></ul><ul><ul><li>3 moles H 2 1 mole N 2 2 mol NH 3 </li></ul></ul>
    5. 5. <ul><ul><li>N 2 ( g ) + 3H 2 ( g )  2NH 3 ( g ) </li></ul></ul>Use a mole ratio to convert between two different compounds in a balanced equation! <ul><ul><li>Some mole ratios: </li></ul></ul><ul><ul><li>1 mole N 2 3 moles H 2 1 mole N 2 </li></ul></ul><ul><ul><li>3 moles H 2 1 mole N 2 2 mol NH 3 </li></ul></ul>
    6. 6. <ul><li>STOICHIOMETRY </li></ul><ul><li>You need a balanced equation. </li></ul><ul><li>Convert the given quantity to moles if needed. </li></ul><ul><li>Convert moles of given compound to moles of another compound by using the mole ratio from the balanced equation. </li></ul><ul><li>Convert moles to grams if needed </li></ul>N 2 + 3H 2  2NH 3 .6mol N 2 x ________ 1mol N 2 2mol NH 3 = 1.2mol NH 3 These numbers come from the balanced equation
    7. 7. for Sample Problem 12.2
    8. 8. <ul><ul><ul><li>For Stoichiometry– </li></ul></ul></ul><ul><ul><ul><li>You ALWAYS use moles!! </li></ul></ul></ul><ul><ul><ul><ul><ul><li>If you are not given moles you must convert to moles. </li></ul></ul></ul></ul></ul><ul><ul><ul><li>Use the mole ratio to convert between compounds. </li></ul></ul></ul>
    9. 9. <ul><ul><li>1. How many moles of water are produced when 2.5 mol of O 2 react according to the following equation? </li></ul></ul><ul><ul><ul><ul><li>C 3 H 8 + 5O 2  3CO 2 + 4H 2 O </li></ul></ul></ul></ul><ul><ul><ul><li>2.0 </li></ul></ul></ul><ul><ul><ul><li>2.5 </li></ul></ul></ul><ul><ul><ul><li>3.0 </li></ul></ul></ul><ul><ul><ul><li>4.0 </li></ul></ul></ul>

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