Chemical Quantities
MAJOR POINTS:
1. unbalanced/balanced
2. conversion (know SI prefix conversion) g-->mol mol-->g or mol--> atom and atom--> mol
3. naming the polyatomics
4. solubility rule
Mole to mole relationship
-all mole to mole relationship comes from balance equation
-it is important to recognize that the coefficients in a balanced equation give us the relative numbers of molecules
-the procedure of rebalancing the equation to obtain the number of moles involved in a particular situation always work.
-we use mole ratios based on the balanced chemical equation
Mass Calculations
-this section we will review the procedures for converting between moles and mass and how these procedures are applied to chemical calculations
using mass-mole conversions with mole ratios- first we would need to balance the reaction that was given. Second, the given number of grams of the compound must be converted into moles. Third, we can use the coefficients in the balanced equation to determine the moles of the compound required.
Lastly, we will use the molar mass of the compound to calculate the grams of the other compound.
using scientific notation- we can balance the equation of 2LiOH(s) + CO2(g)---->Li2CO3(s) + H2O(l)
then we convert the given mass of LiOh to moles using the molar mass of LiOH which is 6.941g +1.008g=23.95g
third step is using the mole ratio which is 1molCo2/2molLiOh. Fourth, is using the mole ratio, we can calculate the moles of CO2 need to react with the given mass of LiOH. Lastly, we can calculate the mass of CO2 by using its molar mass of 44.01g.
the concept of Limiting reactants - limiting reactants is basically the lowest number between the finding the two calculations on finding out 2 different compounds using the same number of grams from a different compound.
calculations involving a limiting reactant- for example, the calculation of methane limits the amount of products that can be formed. The methane that is mixed with water the methane will be consumed before the water runs out. therefore, the water will be in excess.
percent yield- the actual yield of the product is the amount of the product actually obtained, is often compared to the theoretical yield.
actual yield/theoretical yield x 100.
1. unbalanced/balanced
2. conversion (know SI prefix conversion) g-->mol mol-->g or mol--> atom and atom--> mol
3. naming the polyatomics
4. solubility rule
Mole to mole relationship
-all mole to mole relationship comes from balance equation
-it is important to recognize that the coefficients in a balanced equation give us the relative numbers of molecules
-the procedure of rebalancing the equation to obtain the number of moles involved in a particular situation always work.
-we use mole ratios based on the balanced chemical equation
Mass Calculations
-this section we will review the procedures for converting between moles and mass and how these procedures are applied to chemical calculations
using mass-mole conversions with mole ratios- first we would need to balance the reaction that was given. Second, the given number of grams of the compound must be converted into moles. Third, we can use the coefficients in the balanced equation to determine the moles of the compound required.
Lastly, we will use the molar mass of the compound to calculate the grams of the other compound.
using scientific notation- we can balance the equation of 2LiOH(s) + CO2(g)---->Li2CO3(s) + H2O(l)
then we convert the given mass of LiOh to moles using the molar mass of LiOH which is 6.941g +1.008g=23.95g
third step is using the mole ratio which is 1molCo2/2molLiOh. Fourth, is using the mole ratio, we can calculate the moles of CO2 need to react with the given mass of LiOH. Lastly, we can calculate the mass of CO2 by using its molar mass of 44.01g.
the concept of Limiting reactants - limiting reactants is basically the lowest number between the finding the two calculations on finding out 2 different compounds using the same number of grams from a different compound.
calculations involving a limiting reactant- for example, the calculation of methane limits the amount of products that can be formed. The methane that is mixed with water the methane will be consumed before the water runs out. therefore, the water will be in excess.
percent yield- the actual yield of the product is the amount of the product actually obtained, is often compared to the theoretical yield.
actual yield/theoretical yield x 100.
Calculations
Resources
Websiteshttp://www.youtube.com/watch?v=LQN9lH9WAVQ
http://www.youtube.com/watch?v=rESzyhPOJ7I
Other
http://www.chemteam.info/Mole/Grams-to-Moles.html
http://chemistry.about.com/cs/stoichiometry/a/aa042903a.htm
Activity
http://chemvlab.org/vlab/stoic2.html
http://www.youtube.com/watch?v=rESzyhPOJ7I
Other
http://www.chemteam.info/Mole/Grams-to-Moles.html
http://chemistry.about.com/cs/stoichiometry/a/aa042903a.htm
Activity
http://chemvlab.org/vlab/stoic2.html