Aim: To react NaHCO3 with HCl to form NaCl and two other products and then calculate the mole relationships between NaHCO3 and NaCl and calculate a balanced equation for this reaction. Safety: • Wear safety goggles at all time • Handle all chemicals with care • Use equipment like tongs when handling warm/hot objects • If chemicals are spilt on self‚ wash off immediately • Stand at all times Hypothesis: The NaHCO3 will react successfully with the HCl and will form NaCl‚ H2O and
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(Critical Essay On “Just Lather‚ That’s All” By Hernando Tellez) By Benaiah Trudell Just Dilemmas‚ That’s All AP English 10 “Just Lather‚ That’s All” proves that decisions people make and the dilemmas they end up in reflect largely on their personalities. Decisions show everyone what kind of person you are (enthusiastic‚ depressed‚ anger-deprived‚ intelligent‚ careful
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Fuels Investigation Aim: To find out which fuel gives out the most energy. Planning We will be using 6 different fuels to heat up 100ml of water‚ and find out the changes of the temperature. We will measure the temperatures of the water before and after the experiment. We will burn heat the water for exactly 2 minutes‚ and check the changes in temperature. The change in temperature will allow us to work out the energy given off the fuel by using this formula: Mass of water x 4.2 (water’s specific
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needed to form the I3- complex. In this type of analysis‚ excess iodide is added to the oxidizing agent‚ and the triiodine is titrated with stand thiosulfate. This indirect analysis finds the number of moles of ascorbic acid based on the known number of moles of IO3- and subtracting half the amount of moles of the thiosulfate solution. II: Equations: Iodate with Iodide: IO3- + 8I- + 6H+ 3I3- + 3H2O Thiosulfate with Triiodide 2S2O32- + I3- S4O62- + 3I- Ascorbic Acid with Triiodide
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Mg2+ (aq) + 2Cl- (aq). The major findings of this experiment were that there was a chemical reaction between hydrochloric acid and magnesium‚ and the reaction produced the hydrogen gas. The results also indicated how many moles of hydrogen gas were equal to the amount of moles of magnesium consumed. Procedure Step 1:
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concentration = moles / volume 0.10=moles/0.010 Moles of Cu (NO3)2 (aq) = 0.001 moles Mass of empty bottle = 6.00grams Mass of empty bottle +copper metal =6.05grams Mass of copper metal recovered after the experiment = 0.050 grams Finding moles of copper: Moles = mass/ Mr = 0.050 / 63.55 =0.00079 moles
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Processing Raw Data : Part 1 Equation of the reaction; Mg(s) + 2HCl(ℓ) → MgCl2(aq) + H2(g) no of moles : no of moles of Mg = mass/molar mass = 0.31g___ 24.31g/mol = 0.01275 moles no of moles of HCl = molarity x volume = 1.0M x (25/1000)mL = 0.025 moles heat of reaction will be 0.025 moles as HCL act as the limiting reactant. Enthalpy change of the reaction‚H2 Volume of HCL solution =
Free Thermodynamics Enthalpy Measurement
204.22 g/mol No. of moles of KHP = Mass of KHP used / Molar mass = 0.42 g / 204.22 g/mol = 0.0021 moles Concentration of NaOH = No. of moles / Volume = [0.0021 mol / {(22.50 + 25) / 1000} L] * 100 = 4.4 M Trial 2 Mass of KHP transferred = 0.4139 g Volume of Distilled water = 25 mL Volume of NaOH used = 22.80 mL Molar mass of KHP = 204.22 g/mol No. of moles of KHP = Mass of KHP used / Molar mass = 0.4139 g / 204.22 g/mol = 0.0020267 moles Concentration of NaOH = No. of moles / Volume = [0.0020267
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Stoichiometry of a Precipitation Reaction March 20‚2013 Amber McCollum Introduction Stoichiometry is a branch of chemistry that deals with the quantitative relationships that exist among the reactants and products in chemical reactions To predict the amount of product produced in a precipitation reaction using stoichiometry‚ accurately measure the reactants and products of the reaction‚ determine the actual yield vs. the theoretical yield and to calculate the percent yield. The equation
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Mole Conversion Web Quest EO 103 What the heck is a mole? We have Avagadro ( and others) to thank for this…….. 6.02 x 1023 is the number of “things” per mole of the substance. Here is a tutorial for an over view and for a reference as you work through these problems http://www.wiley.com/college/chem/spencer053872/tutorial/gramsmoles/gramsmoles1.html We can use this to do mathematical conversions to determine mass‚ volume‚ and number of atoms or molecules in a given substance. For example let’s
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