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Stoichiometry: - Coggle Diagram
Stoichiometry:
Quantitative and qualitative Analysis and Chemical Equation Review (L1):
Quantitative:
Qualitative:
Formation
Decomposition:
Single Replacement:
Double Replacement:
Neutralization:
Combustion:
Hydrocarbon combustion:
Acid-Base Titration (L6):
Lab Equipment/material:
Burette: Holds the titrant
Titrant: Can be an acid or a base and is released until the solution is neutralized. Ifi t is a base, the pH starts low, and gradually increases. If it is an acid, the solution has a high pH and slowly decreases.
Erlenmeyer Flask: Holds the analyte
Analyte: Can be an acid or a base. Is measured out before the experiment and the titrant is slowly added to it.
Burette Clamp: Holds the burette.
Retort Stand: Mounts the burette clamp.
Tap/Stop Cock: Controls the release of titrant.
Equivalence point: The point at which just enough titrant has been added to neutralize the analyte. The first/initial drop added that neutralizes the solution and the indicator changes color. (once the endpoint has been reached_
Endpoint: The point in which the indicator changes color.
Standardization: Determining the concentration of the solution.
pH: If the solution is neutralized the pH is 7 or close to 7.
Indicator: The substance added to the solution that changes color when it is neutralized.
Titration Curve: look on graph, P.g. 21
Mole Ratio and Stoichiometry Intro (L2):
Gravimetric Stoichiometry:
Solutions Stoichiometry:
Gas Stoichiometry:
Stoichiometry basic Steps: -Balance equation
-Convert to number of moles for given
-Do mole ratio to find moles for required
-Rea-range and do any conversions necessary.
Stoichiometry and Percent Yield (L5):
Predicted Yield: The expected quantity of a product (usually given within a question.)
Experimental Yield: The quantity of the product that is actually obtained within a reaction. (The number you solved for in a equation)
Factors Affecting Experimental Yield:
Competing Reactions: Sometimes, multiple reactions can occur within the same solution and they compete with each other.
Slow Reactions: If not enough time has been given for the reaction to occur (beacuse it is slow), the experimental yield may not be fully obtained.
Collection and Transfer Methods: During transfer of reactants or solution, parts of product may be lost.
Reactant purity: Reactants may have contaminant in them.
Reactions that don't proceed to completion: Reactions may reach an endpoint even though not all reactants have been used.
Calculating Percent Yield: Percent Yield = Experimental Yield x 100 / Predicted Yield.
Note that smaller number is on the top. Experimental yield is the actual yield that you found when solving and the predicted will always be given.
Solution and Gas Stoichiometry (L3):
Solutions Stoichiometry Steps: -Balance the equation
-Write down all the givens
-Find the number of moles for the given
-Convert the given to the required using mole ratio
-Do any other calculations required E.g. Converting the required's number of moles to mass.
Gas Stoichiometry Steps: -Write a balanced chemical equation -If all gases are found at the same temp and pressure, use the law of combining volumes (PV = nRT) - If only one substance is a gas, or there is a change in temp or pressure, use ideal gas law (P1V1/T1 = P2V2/T2)
Stoichiometry and Ideal Gas Law:
Limiting reactant and Expected Yield (L4):
Limiting Reactant: The reactant that is completely consumed/used with a reaction. Its called the limiting reaction because as soon as it is used up the reaction stops and it limits the use of all other reactants.
Solving For the Limiting Reactant Steps: -Write your balanced equation
-Find number of moles for both reactants and convert them to the precipitate.
-The conversion that results with the smaller number of moles correlates with the limiting reactant.
Finding Excess/left-over reactants (steps): -Balance the equation
-Collect given then find the number of moles for both reactants.
-Convert to the precipitate to find the limiting reactant (smaller number is the limiting reactant)
-Use both number of moles and subtract the excess reactant (bigger number) by the limiting reactant (smaller number) to find the difference in moles.
Simply convert the difference in moles back to excess reactant to find how much is left over.
-Do any conversions necessary if asked.