Day 3 of the lab.
Today we finished weighing the mass of the jar and copper and calculated the % yield to determine the charge of the Iron. First we subtracted the original mass to the new mass of the nail after the reaction and did the same with the copper (jar+copper-jar mass) to get how much copper was left. We then converted the mass of the iron into copper to get the theoretical yield which was over 100%, if the iron was a 2+ charge, and a little over 70% if calculated at 3+ leading us to believe that the Fe was a 3+.
Here's some more information on finding the theoretical yield. Tripod
Monday, December 14, 2015
Sunday, December 13, 2015
Post 3 Stoichiometry
Day 2 of the lab.
After the nail has reacted over night, we pulled it out and proceeded to wash and rinse the whole jar while making sure to avoid losing any copper through the process as this will be needed to determine if our element has a 2+ or 3+ charge. We are now allowing the remainder of the liquid to fully dry before we begin weighing the copper.
After the nail has reacted over night, we pulled it out and proceeded to wash and rinse the whole jar while making sure to avoid losing any copper through the process as this will be needed to determine if our element has a 2+ or 3+ charge. We are now allowing the remainder of the liquid to fully dry before we begin weighing the copper.
Saturday, December 12, 2015
Post 2 Stoichiometry
Day 1 of the lab.
Today we placed 4 grams of copper II chloride, CuCl2, into a baby food jar, added 50mL of water and stirred. The water became a bright, pretty blue. We then, after polishing, placed an iron nail inside which immediately began collecting the copper into a rusted red substance.
Here's a worksheet that further explains the lab. quia
Today we placed 4 grams of copper II chloride, CuCl2, into a baby food jar, added 50mL of water and stirred. The water became a bright, pretty blue. We then, after polishing, placed an iron nail inside which immediately began collecting the copper into a rusted red substance.
Here's a worksheet that further explains the lab. quia
Wednesday, December 9, 2015
Post 1 Stoichiometry
Stoichiometry is our next unity that involves finding the relationships, measurements, between reactants and products within a chemical reaction. It begins with balancing the equation, finding the molar mass of the reactant then converted to mols, using the coefficients (mols) of the reactant to the converted product, and then converting the mols of the new product back to mass (grams).
Using this same method, you can use stoichiometry to find the limiting reagent within a reaction by calculating each of the reactants using the same conversion method as described above, converting it into the product, and then finding which produces the least amount of product using the given mass. This is the LR which can only produce so much of the product leaving the other reactant with excess.
When determining the excess reactants left over, use the amount of product created with the limiting reactant and convert it using the same formula as stated before into the excess reactant to find how much of that element (species) was used up in the chemical reaction. Then subtract this answer from the original mass of that reactant that you began with to find how much was not used in the reaction (or left over). This is your excess.
Finally, stoichiometry is also used with the chemical equation Yield% = 100X(actual yield/theoretical yield)
When doing all of these formulas, make sure the equation is balanced and the only transition of elements can be calculated through mols.
Here's some sites that may help.
khanacademy
CrashCourse
chemwiki
chemteam
Using this same method, you can use stoichiometry to find the limiting reagent within a reaction by calculating each of the reactants using the same conversion method as described above, converting it into the product, and then finding which produces the least amount of product using the given mass. This is the LR which can only produce so much of the product leaving the other reactant with excess.
When determining the excess reactants left over, use the amount of product created with the limiting reactant and convert it using the same formula as stated before into the excess reactant to find how much of that element (species) was used up in the chemical reaction. Then subtract this answer from the original mass of that reactant that you began with to find how much was not used in the reaction (or left over). This is your excess.
Finally, stoichiometry is also used with the chemical equation Yield% = 100X(actual yield/theoretical yield)
When doing all of these formulas, make sure the equation is balanced and the only transition of elements can be calculated through mols.
Here's some sites that may help.
khanacademy
CrashCourse
chemwiki
chemteam
Wednesday, December 2, 2015
Post 5 Chemical Reactions
Yesterday we did the lab which included single replacement reactions by combining chemicals and elements. Some of the reactions resulted in smoking, fizzing, and change in coloration which was all interesting to see.
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