Exam Review Sheet #1 Balancing Equations and Simple Stoichiometry Answers are provided on the second sheet. Please try to do the worksheet without referring to them‚ because you’ll be expected to know this stuff the first day of school! Balance the following equations: 1) ___ N2 + ___ F2 ( ___ NF3 2) ___ C6H10 + ___ O2 ( ___ CO2 + ___ H2O 3) ___ HBr + ___ KHCO3 ( ___ H2O + ___ KBr + ___ CO2 4) ___ GaBr3 + ___ Na2SO3 ( ___ Ga2(SO3)3 + ___ NaBr 5) ___ SnO + ___ NF3 ( ___ SnF2
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Name: Exp 9: Stoichiometry of a Precipitation Reaction Data Tables: Step 3: Show the calculation of the needed amount of Na2CO3 CaCl2.H2O(aq)= m/M =1/147 =0.0068 mol CaCO3(s)=0.0068*1/1 =0.0068 mol CaCO3 (s)= CaCO3 mol *CaCO3 g =0.0068 mol*100.01 g =0.68 g Convert moles of Na-2CO3 to grams of Na2CO3 = 0.00680 moles Na-2CO3 x 105.99g Na-2CO3 1 mole Na-2CO3 = 0.72g 0.72g of Na-2CO3 to fully react with 1g of CaCl2-.2H2O Step 4: Mass of weighing dish
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Aspirin and salicylic acid have similar properties‚ but many choose aspirin for medicine because it is not as acidic as salicylic acid. The limiting reagent limits how much product can be synthesized. Once
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in distilled water and then mixed them together in a single beaker. Finally we filtered this mixture and let all the water evaporate leaving behind solely the precipitate. In order to determine the amounts needed of each reactant we had to use stoichiometry. First we had to set up a balanced equation of the precipitate reaction that yielded 2.00 grams of CaCo3‚ then we looked at the ratio of moles reactant to moles product. We then substituted the ratio of the molar mass of each reactant to molar
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Chemistry June Exam Notes Quantities in Chemical Reactions Molecular and formula mass o The mass of one unit of a compound (a molecule or a formula unit) o The sum of the mass of all the atoms in a compound o With knowledge of the mass of each individual atom‚ the percentage composition by mass can be determined The Mole (mol) o A counting unit‚ one mole refers to 6.02 x 1023 particles of any given substance o Known as Avogadro’s Constant and given the symbol NA Molar Mass o The
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Table of reagents Name Density (g/ml) Amount used Amount # moles Bromine (excess) Trans-cinnamic Acid 1.246 g/cm3 0.148g – do conversion Dichloromethane 1‚3266 g/cm3 - Table of Results Name Amount obtained Molar Mass (g/mol) Amount used (moles) Melting point (Celsius) Color/observations 2‚3-dibromo-3-phenylpropanoic acid 0.285g 307.97 200.4 – 205.1 White powder Limiting reagent: Trans-cinnamic acid (148.16g/mol) 2.5g/148.16g/mol=0.01687mol Stoichiometry ratio: 1:1 ratio
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AP Chemistry Final Exam Review ESSAY. Write your answer in the space provided or on a separate sheet of paper. 1) Explain the difference between a qualitative and a quantitative measurement. Provide examples to illustrate this difference. Answer: A qualitative measurement is a measurement that gives descriptive‚ nonnumeric results; a quantitative measurement is a measurement that gives definite‚ usually numeric results. "The rock is heavy" would be a qualitative measurement. "The rock weighs 110
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Compound Amount used MW (g/mol) Moles Stoichiometry/Comments acetaminophen 0.354 g 151.16 2.34 x 10-3 limiting reagent ethyl iodide 0.3mL 155.97 3.75 x 10-3 1.6 equiv ’s sodium ethoxide 2.6mL 68.05 3.3 x 10-2 catalyst‚ reaction solvent crude product obtained: phenacetin 0.32g 179.22 1.78 x 10-3 yield = 76.06% Recrystallized product: phenacetin 0.16g 179.22 8.92 x 10-4 yield = 38.12% Table 1-Reagent and yield Data for the synthesis of Phenacetin Calculations
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Title: Double Replacement Reactions (Data and Calculations) Objective: Classify the chemical reaction through observation‚ which each reagent produce when mixed with another reagent. After careful observation‚ be able to prove each observation using the net ionic equation. Background: First‚ a double-replacement reaction is when two cations in different compound switch anions‚ AX + BZ → BY. If either compounds are insoluble a precipitate occurs‚ and if there is no precipitate formed there is
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equation was 2NaHCO3(S) > Na2CO3(s) + CO2(g) + H2O(g). The procedure consisted of gathering measurements and observing. The first step was to gather all the necessary materials. Next we had to have the accurate measurements of the crucible with and without the substance that is Sodium bicarbonate. The Crucible had a mass of 11.53g and then 13.94g with Sodium bicarbonate. Subtracting it to find out the
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