The absorption spectrum is measured using a spectrophotometer and the data is graphed in Excel. The peak of the line is used to find Vmax of Fe2+. Vmax is used to find the moles of Fe2+ and ligand. The unknown n is a ratio of moles ligand divided by moles Fe2+. Results and Discussion For the first part of the experiment (Part A), five different 100 mL volumetric flasks were each filled with 1,2,3,4 and 5 mL of iron (II) solution.
Record the mass of thyme used. 2. Using a measuring cylinder, add 50cm3 of 1.0mol dm-3 sulphuric(VI) acid and boil gently for 5 minutes. 3. Allow the mixture to cool for a few minutes then filter it, using either gravity or vacuum filtration.
Nest two Styrofoam cups within one another 2. Turn on magnetic stirrer 3. Insert probe into cardboard lid 4. Pour 25mL of water into calorimeter 5. Determine initial temperature of water 6.
All color observations were recorded and compared to the known behaviors of the focus metals. The next step to identifying the unknown compound solution involved chromatography. Two 20 x 10 cm pieces of chromatography paper were obtained, both labeled six times: five for each individual metal sample and one for the unknown sample. A capillary tube was then used to spot all samples onto their appropriate positions on both pieces of paper. Each paper was then rolled, stapled on the top to create a tube, and carefully placed into a 600mL beaker, one containing ~30mL of 6M HCl, the other containing ~30mL of 1.5M HCl.
This is because Bentonite clay has adsorbing abilities due to its molecular shape. It has a large area that allows other molecules to adhere to it by the process of intercalation. A way to test this theory is with spectrophotometry. By obtaining the absorption spectrum of a red dye containing PAHs, one can compare that absorption to the absorption of the dye after Bentonite clay has been used to remove PAHs. Materials and Methods: To begin the experiment, the Bentonite clay had to be made.
Record the readings of the three instruments at eight different speed settings of the tunnel: 15, 20, 25, 30, 35, 40, 45, & 50. 4. Plot two calibration curves with pressure transducer reading as the abscissa and micromanometer reading as the ordinate for the first, and micromanometer versus scannivalve as the second. Convert micromanometer data to read as total pressure in SI units [Pa]. 5.
5.04H: Gas Stoichiometry Lab Worksheet Name: _________________________ Data and Observations: Present all relevant data in a data table below. Include an observations section for any observations that you made during the lab. (5 points) Data Table| Mass of magnesium strip (grams)|0.0304g| Volume of gas collected (mL)|10ml| Barometric pressure (atm)|1.1| Room Temperature (°C)|21 | Vapor pressure of the water (torr)|18.7| Calculations: 1. Write the balanced equation for the reaction conducted in this lab, including appropriate phase symbols. (2 points) Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq) 2.
Homework Unit 57 Section 7 1. What friction rate should be used to size a duct for a static pressure drop of 0.1 in wc if the duct has a total equivalent length of 150 ft? (57.10) 2. What size metal duct should be used to deliver 170 CFM with a pressure drop of 0.15 in wc if the total equivalent length of 130 ft? (57.10) 7 in.
Materials and Methods The experiment was started by setting up a Spec 20 spectrophotometer and collecting materials such as glassware, stirring rods, and thermometers to mix solutions containing Bromothymol Blue. Approximately .416 grams of Na2HPO4 and .409 grams of NaH2PO4 were dissolved with 50mL of distilled water in a 150mL breaker to create a buffer solution. Twenty drops of 0.04% Bromothymol Blue were added to the solution and the pH was measured to be exactly 7 using a Vernier probe. 5mL of solution was then distributed to three 100mL beakers using a volumetric pipette. Each beaker was filled with either 1mL of 1.0 M HCl, 1mL of 1.0 M NaOH, or 1mL of water with a pipette, in order to create three solutions that had varying pH levels.
Calculate the value of Ke for this system. 2 H2S (g) === 2 H2 (g) + S2 (g) [1.1(10-4] 7. At a given temperature, the following system has an equilibrium constant, Ke, of 0.27. C(g) + B(g) === 2 E(g) The system was established by placing 8.00 moles of C and 5.0 moles of B in a 4.0 L vessel. Calculate the concentration of all substances at equilibrium.