Lab Report 9 Bleach Oxidation Essays

In the first part of the lab, the goal of this experiment was to carry out an oxidation of diphenylmethanol

The formula came out to be MgO, because 1.16 is rounded to 1 and 1 is not written in the

(0.074 mol HCl x 1 mol NaOH) / 1 mol HCl = 0.074 mol NaOH

Your mass precision should be reported to a thousandth of a gram, i.e. 0.302. (Use 3 significant figures.)

8. Repeat step 7 with H2SO4, except that you should use a 10 mL graduated cylinder of H2SO4 and adding 15 mL water.

peroxide there is in 5.0mL of the reacted solution; to figuring out exactly how much

Approximately 0.05 g of 9-fluorenol, 250mg of chromic oxide resin, and 2 mL of toluene were used for the reaction solution. The CrO3 resin consisted of little brown solid balls. The reaction solution was slowly heated to 130°C. The reaction solution slowly turned light yellow as it was being heated. 1M standards for 9-fluorenol and 9-fluorenone were used. The reaction mixture had a strong gas-like odor while it was filtered through the Hirsch funnel. After evaporating the solvent using a rotary evaporator, the crude product that was left was yellow and solid. When hexane was added the yellow solid formed into a yellow liquid.

In order to calculate this value, the moles of anthranilic acid were needed, since it was the limiting reactant. The mole for anthranilic acid was 0.01456 mol. We then had to calculate the theoretical yield, which in this case was 2.614g. This was obtained by multiplying the moles of anthranilic acid with the molar mass of N-acetylanthranilic acid as well as multiplying the mole ration of 1:1, thus obtaining the value 2.614g. Finally, we had to divide the mass of the purified product with the theoretical yield and multiply it by 100 in order to get 16%. This percent yield was incredibly low, however we did mass the crystal after taking the melting point, which of course altered our data—thus bringing us to a low percent yield. Next time we will mass the product before doing other activities that could alter our mass.

The most common fluorine minerals are fluorite, fluorspar and cryolite (Fluorine). Fluorine is also the 13th most common element in the Earth’s crust (Fluorine). There is 950 mg/L of fluorine in the earth’s crust (Periodic). Fluorine is also in seawater. Around 2,400 tons of fluorine gas and 4,700,000 tons of fluorite are produced each year (Periodic). Fluorine production areas are primarily in Canada, United States, United Kingdom, Russia, Mexico and Italy (Periodic). Fluorine is most commonly combined with sodium to form sodium fluoride (NaF) to put into toothpaste (Periodic). A very interesting fact about fluorine is that it is added to city water supplies in the proportion of about one part per million to help prevent tooth decay (The Element). Hydrofluoric acid is used to etch glass, including most of the glass that is used in light bulbs (The Element). You cannot purchase straight fluorine due to it being highly

Does Bleach Eliminate Bacteria? Abstract There are many methods used to destroy bacteria and this experiment tests the affects of Clorox bleach on bacteria. It will outline the methods used to determine if bleach could, or should be, used to decrease the amount of bacteria and whether or not this particular method is effective. The experiment will also test whether the levels of phosphorus and phosphatase in the soil are affected.

This report concerns the experiment of determining the order of reaction and the kinetic rate constant of alcohol oxidation. This experiment relates to the knowledge of chemical kinetics, the application of Beer’s Law, and other calculations.

In this equation shown above, our trial three our molarity ended up as 0.63716014 M and our molality ended up being 8.18627m.

The chemical reaction being: Zn (s) + 2HCl (aq)—> ZnCl2 + H2 and calculating the amount of .1167 through a stoichiometric calculation (which can be seen as calculation two in the calculation

Introduction: In this lab we will observe the rate of ethanol oxidation and determine the rate constant that correspond to it. The rate law for this experiment can be written as: rate= k 〖[〖〖Cr〗_2 O_7〗^(-2)]〗^x 〖[C_2 H_5 OH]〗^y where x and y are both the partial order of the reactant in a reaction and k is the kinetic rate constant.

0.210 x 345.929 = 7.277 g (moles x Mr of Ni (C2 H8 N2) 3 2+ Cl2·2H2O)