One of the reactions you observed resulted in this product: NaCl + H2O + CO2 (g)? What well did this reaction occur in? Describe how the observations for this reaction support your answer. B BoldI ItalicsU Underline Bulleted list Numbered list Superscript Subscript70 Words A reaction I observed in number 1.) Sodium Bicarbonate mixed with Hydrochloric acid.
For example, an experiment similar to this one could be how pressure could affect the time it takes for an Alka-Seltzer tablet to dissolve. Using A flask and rubber stoppers, you can compare the amount of time it takes for and Alka-Seltzer tablet to dissolve in regular room temperature water and room temperature water in a flak but with a rubber stopper stopping the air flow into the flask. This is related to the experiment performed above because the increase in pressure from the rubber stopper stopping the air flow in and out of the flask may affect the time it would take for the Alka-Seltzer tablet to dissolve. Another example of an experiment related to the one performed above is how the amount of water used to dissolve an Alka-Seltzer tablet effects the time it takes for one to dissolve. This also relates to the experiment performed above because it also affects how fast the rate of reaction is.
The supernatant was assayed for SOD activity by following the inhibition of epinephrine auto-oxidation. 0.5ml of sample was diluted with 0.5 ml of distilled water, to this 0.25 ml ethanol, 0.5 ml of chloroform (all reagents chilled) was added. The mixture was shaken for 1 min and centrifuged at 2000 rpm for 20 min. The enzymatic activity in supernatant was determined. To 0.05 ml of carbonate buffer (0.05 M, pH 10.2) and 0.5 ml of EDTA (0.49 M) was added.
The goal of the experiment is to synthesize a bromohexane compound from 1-hexene and HBr(aq) under reflux conditions and use the silver nitrate and sodium iodide tests to determine if the product is a primary or secondary hydrocarbon. The heterogeneous reaction mixture contains 1-hexene, 48% HBr(aq), and tetrabutylammonium bromide and was heated to under reflux conditions. Heating under reflux means that the reaction mixture is heated at its boiling point so that the reaction can proceed at a faster rate. The attached reflux condenser allows volatile substances to return to the reaction flask so that no material is lost. Since alkenes are immiscible with concentrated HBr, tetrabutylammonium bromide is used as a phase-transfer catalyst.
1 “substrate” and another “ enzyme.” Instead of using the distilled water, this time you are going to use different pH buffer in the enzyme test tube. In the substrate tube, add 7 mL of distilled water, 0.3 mL of hydrogen peroxide, and 0.2 mL of guaiacol for a total volume of 7.5 mL. For the enzyme tube, instead of distilled water add the pH solution (3) and 1.5 mL of peroxidase which equals a total volume of 7.5 mL. Use the dH2O syringe for our pH solution. To clean the syringe, flush it by drawing 6 mL of distilled water.
Throughout the experiment, there was a struggle to keep the heat stable which led to inaccurate data. Additionally, while changing the receiver from cyclohexane to toluene there was a loss of distillate which also led to the errors observed in the data. Furthermore, if more data were collected for each compound it would be a better representation of the experiment's results. If these errors were avoided, then the experiment would be more efficient in distilling the two compounds from each other and the plateau would be as sharp as figure 6 in the lab
The volume of the water was not taken into account due to the priority of adjusting the temperature of the water. The lack of consistency in the amount of water may have affected the reaction time, since more coverage of the hand with water will facilitate the process of warming the hand. When there is a larger amount of water in the plastic tub, more surface area of the hand will be submerged by the water. In addition, the hand will be more influenced by the temperature of the water when more surface area of the hand is in contact with the water. One solution is to keep the volume of the water consistent.
Their different molecular conformations give them different. inter-molecular packing. These forms are created by controlling the crystallisation supersaturation. The α form is less stable than the β form because α amino groups are directed towards the crystals surface while the carboxyl remains below. From theory the α The longer the β crystal is allowed grow in solution at a high temperature the more stable it becomes due to its changing lattice.
Thus, the amount of the carbon dioxide collected in measuring cylinder will be affected, causing the rate of reaction to be altered. In addition, the source of the random errors in this experiment is the widely spaced graduation mark on the 100mL measuring cylinder, result in variation in the eye level to determine the amount of carbon dioxide released and the amount of diluted hydrochloric acid used which may lead to the rate of reaction changes irregularly as the time taken to collect 30cm³ of carbon dioxide is affected. Equally important, the air movement in the room will also affect the rate of reaction as the air movement will affect the temperature, thus indirectly affect the rate of reaction. When magnesium carbonate reacts with hydrochloric acid, this is an exothermic reaction where heat will be release out and increases the rate of reaction. However, air movement in the room causes the advection of heat.
Results With Respect to Potassium Bromate(V) The table below shows my results when varying the concentration of potassium bromate(V): ￼ ￼ ￼ Concentration of Potassium Bromate(V) (mol/dm-3) Time Take For the Mixture to Turn Colourless (seconds) ￼ ￼ ￼￼￼￼￼￼ Trial 1 Trial 2 Trial 3 Trial 3 Trial 5 Average Reaction Rate (seconds-I) ￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼ ￼￼￼￼￼￼ 0.01 31.9 ±0.01 32.2±0.01 31.7±0.01 31.8±0.01 32.0±0.01 31.92±0.05 0.0313 ￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼ ￼￼￼￼￼￼ 0.008 45.6±0.01 45.1±0.01 45±0.01.3 45.4±0.01 45.2±0.01 45.32±0.05 0.0221 ￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼ ￼￼￼￼￼￼ 0.006 62.8±0.01 63.4±0.01 ±0.0162.7 62.9±0.01 6±0.013.2 63.00±0.05 0.0159 ￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼ ￼￼￼￼￼￼ 0.005 88.8±0.01 88.3±0.01 89.0±0.01 88.5±0.01 88.7±0.01 88.66±0.05 0.0113 ￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼ ￼￼￼￼￼￼ 0.004
My group recorded higher heart rate compare to the class average when we used caffeine on the Daphnia as seen in Figure 2. Several errors could have accounted for this data. This including perhaps the Daphnia’s heart rate may have changed because of fear while being moved from the bowl to the microscope slide. Another possible error could have also been the amount of time that it took to change the solutions, which could have accounted for slight variations in heart rate. Temperature is yet a further error to account for as the microscope slide temperature was constantly changing to view the specimen, and change the dosage of caffeine or alcohol.
The topic of research is, “how fast does an Alka-Seltzer tablet make gas?”. In the experiment, the scientists will be measuring the chemical reaction rates that occur, when 1 Alka-Seltzer tablet is placed in a specific temperature of water. The independent variable during the experiment will be the temperature of the water (degrees Celsius). The dependent variable during the experiment will be, the rate in which gas is produced (in seconds). The constants of the experiment, will be the amount of water used and the Alka Selter compound.
Name: University: Course: Date: Abstract I. Introduction/Motivation: The objective of this experiment was to characterize the behavior of a distillation column running in continuous mode. Two types of liquids were separated: 2-propanol and methanol (at 25 mol% and 75 mol% respectively). The motivation of this investigation was to achieve 85% of methanol recovery from the distillate. II. Methodology: The distillation column was analyzed theoretically using McCabe Thiele to establish the number of stages required for separation.