Your SlideShare is downloading. ×
0
Stoichiometry
Stoichiometry is thestudy of quantitative   relationships inchemical reactions.
The basic idea used insolving stoichiometric problems is the mole       concept.
A short review
Molecular weight is the  sum of the atomicweights of all the atoms    in a molecule.  A molecule is the  smallest unit of ...
What is a mole?
A mole (mol) is a SI baseunit used to measure the amount of material in a    chemical sample.
1 mole of H2O contains6.022 x 1023 H2O molecules   (Avogadro’s number)
A coefficient in a balanced chemical equation indicates   the number of moles of achemical compound involved in     a chem...
The coefficients give you themole ration of the compounds  involved in the reaction.       2H2 + O2  2H2O The mole ratio ...
The unit of moles  provides a “bridge” to mathematically convertbetween several different   aspects of chemical       comp...
Moles link an abstractchemical equation to a   concrete unit ofmeasurement (grams,  Liters, number of     molecules)
For example:1 mole = 6.02 x 1023 molecules1 mole = molecular mass of a         substance1 mole = 22.4 L of a substanceat S...
For example:1 mol Cl = 6.02 x 1023 molecules Cl 1 mol H2O = 6.02 x 1023 molecules                H 2O       1 mol Cl = 35....
There are several types of calculations that can be  used in Stoichiometry.
Mole – molecalculations
Involves 1conversion  factor
The object of this type ofproblem is to calculate the  moles of one substancewhen given the number of    moles of differen...
Example: Magnesiumhydroxide reacts with carbonicacid. How many moles of water     will be produced from    3.5 moles of ma...
Example: How many molesof ammonia can be producedfrom 8.00 moles of hydrogen   reacting with nitrogen?
Example:K2Cr2O7 + 6KI + 7H2SO4  Cr2(SO4)3 + 4K2SO4 + 3I2 + 7H2O    Calculate the number of moles of      potassium dichro...
Mole – mass calculations
Involves 2conversion  factors
The object of this type of  problem is to calculate     the moles of onesubstance when given the     mass of different    ...
Example:What mass of hydrogen can be    produced by reacting 6.0 moles of aluminum with     hydrochloric acid?    You are ...
Example: How much    carbon dioxide isproduced by the completecombustion of 0.0492 mol    of propane, C3H8?
Example: How many moles of water will be produced from 14.6 g    propane in thecombustion of propane?
Mass – Mass calculations
Involves 3conversion  factors
The object of this type of  problem is to calculate     the mass of onesubstance when given the     mass of different     ...
Example:How much carbon dioxide is produced by the complete      combustion of 100.0 g of propane, C3H8?   You are given t...
Example: Magnesium  chloride reacts withsulfuric acid. How muchsulfuric acid is needed to    produce 26.3 g of  magnesium ...
Calculationsinvolving Liters and number of   molecules
Example: How many molesof ammonia can be producedfrom 1.03 Liters of hydrogen  reacting with nitrogen at            STP?
Example: How many carbon   dioxide molecules are produced by the completecombustion of 32.00 grams     of propane, C3H8?
Stoichiometry for online
Stoichiometry for online
Stoichiometry for online
Stoichiometry for online
Upcoming SlideShare
Loading in...5
×

Stoichiometry for online

568

Published on

0 Comments
0 Likes
Statistics
Notes
  • Be the first to comment

  • Be the first to like this

No Downloads
Views
Total Views
568
On Slideshare
0
From Embeds
0
Number of Embeds
0
Actions
Shares
0
Downloads
13
Comments
0
Likes
0
Embeds 0
No embeds

No notes for slide

Transcript of "Stoichiometry for online"

  1. 1. Stoichiometry
  2. 2. Stoichiometry is thestudy of quantitative relationships inchemical reactions.
  3. 3. The basic idea used insolving stoichiometric problems is the mole concept.
  4. 4. A short review
  5. 5. Molecular weight is the sum of the atomicweights of all the atoms in a molecule. A molecule is the smallest unit of a covalent compound.
  6. 6. What is a mole?
  7. 7. A mole (mol) is a SI baseunit used to measure the amount of material in a chemical sample.
  8. 8. 1 mole of H2O contains6.022 x 1023 H2O molecules (Avogadro’s number)
  9. 9. A coefficient in a balanced chemical equation indicates the number of moles of achemical compound involved in a chemical reaction. 2H2 + O2  2H2O
  10. 10. The coefficients give you themole ration of the compounds involved in the reaction. 2H2 + O2  2H2O The mole ratio of hydrogen to oxygen is 2:1 (for every oneoxygen put into the reaction, 2 moles of hydrogen are alsoneeded to put into the reaction)
  11. 11. The unit of moles provides a “bridge” to mathematically convertbetween several different aspects of chemical compounds.
  12. 12. Moles link an abstractchemical equation to a concrete unit ofmeasurement (grams, Liters, number of molecules)
  13. 13. For example:1 mole = 6.02 x 1023 molecules1 mole = molecular mass of a substance1 mole = 22.4 L of a substanceat STP (standard temperature and pressure)
  14. 14. For example:1 mol Cl = 6.02 x 1023 molecules Cl 1 mol H2O = 6.02 x 1023 molecules H 2O 1 mol Cl = 35.45g Cl 1 mol H2O = 18.01g H2O 1 mol Cl = 22.4L Cl @ STP 1 mol H2O = 22.4L H2O @ ATP
  15. 15. There are several types of calculations that can be used in Stoichiometry.
  16. 16. Mole – molecalculations
  17. 17. Involves 1conversion factor
  18. 18. The object of this type ofproblem is to calculate the moles of one substancewhen given the number of moles of different substance.
  19. 19. Example: Magnesiumhydroxide reacts with carbonicacid. How many moles of water will be produced from 3.5 moles of magnesium hydroxide? You are given the moles of one substance and asked to find the moles of another substance.
  20. 20. Example: How many molesof ammonia can be producedfrom 8.00 moles of hydrogen reacting with nitrogen?
  21. 21. Example:K2Cr2O7 + 6KI + 7H2SO4  Cr2(SO4)3 + 4K2SO4 + 3I2 + 7H2O Calculate the number of moles of potassium dichromate that will react with 2.0 moles of potassium iodide. Calculate the number of moles of iodine that will be produced from 2.0 moles of potassium iodide.
  22. 22. Mole – mass calculations
  23. 23. Involves 2conversion factors
  24. 24. The object of this type of problem is to calculate the moles of onesubstance when given the mass of different substance. Or vise versa
  25. 25. Example:What mass of hydrogen can be produced by reacting 6.0 moles of aluminum with hydrochloric acid? You are given the moles of one substance and asked to find the mass of another substance.
  26. 26. Example: How much carbon dioxide isproduced by the completecombustion of 0.0492 mol of propane, C3H8?
  27. 27. Example: How many moles of water will be produced from 14.6 g propane in thecombustion of propane?
  28. 28. Mass – Mass calculations
  29. 29. Involves 3conversion factors
  30. 30. The object of this type of problem is to calculate the mass of onesubstance when given the mass of different substance.
  31. 31. Example:How much carbon dioxide is produced by the complete combustion of 100.0 g of propane, C3H8? You are given the moles of one substance and asked to find the mass of another substance.
  32. 32. Example: Magnesium chloride reacts withsulfuric acid. How muchsulfuric acid is needed to produce 26.3 g of magnesium sulfate?
  33. 33. Calculationsinvolving Liters and number of molecules
  34. 34. Example: How many molesof ammonia can be producedfrom 1.03 Liters of hydrogen reacting with nitrogen at STP?
  35. 35. Example: How many carbon dioxide molecules are produced by the completecombustion of 32.00 grams of propane, C3H8?
  1. A particular slide catching your eye?

    Clipping is a handy way to collect important slides you want to go back to later.

×