The observed emission data for the different elements did not look how they were supposed to. However the “peaks” for Hydrogen were found to be 534.52 and 631.24, 534.70 and 569.11 for Helium and 529.73 and 630.71 for Mercury. The Rydberg’s Constant found to 1.1x107 8.5x104 while the known constant is 10967758.34m-1. The percent error of 0.29% and the accuracy of this reading is 99.7. The slope and intercept of the linear regression line is -0.01 3.3x10-5 and 0.02x10-1 1.9x10-6 respectfully.
1. A number of different items were measured in this lab. For each of the following items, what did you find most challenging in making the measurement and how did that challenge affect the accuracy of the measurement? a) Length of the table b) Height of your partner c) Thickness of your finger
Based on your class results is there a correlation between the strength of the acid and the amount of heat given off when it reacts with a base? a) Compare the values of the heats of neutralization for the reactions of each acid with either sodium hydroxide (NaOH) or aqueous ammonia (NH₃). Can you make any correlation between the quantities of the heat given off and the fact that sodium hydroxide is a stronger base than ammonia (NH₃)? A negative ΔH indicates a process giving off heat, making it exothermic.
Intro: Light can act as a wave or a particle, it depends on certain circumstances light can go through. It can interact with different chemicals and telling us what we can see in a solution. Light can show the different types of factors that can occur in the state of the substance such as solid, liquid or gas. Light can be absorbed by objects, which means light must be absorbed by a chemical substance in order for the photoelectric effect to take place. This effect is known for electron being emitted when light is shined upon it and photons may or lose the absorbance.
The freezing point for tert-butanol in literature is 78 F, or approximately 25 C, which is quite close to what was observed, as stated in the Freezing Points Table. (NOAA, 2016). The molarity of the additive substance could be calculated by taking the moles used and diving by the volume of the solvent. So for benzoic acid, there would be two different values.
The following experiment was followed from the handout provided by Dr. Donald A. "Chopper" Krogstad, Professor of Chemistry at Concordia College, Moorhead, Minnesota. First, the calorimetry constant for the specific bomb calorimeter used had to be determine with a molecule that had a known heat capacity. One gram of benzoic acid, and 10 cm of ignition wire were placed in the bomb as described by the handout. The bomb was then sealed with its cover, and connected to a O2 tank. O2 was slowly let into the bomb, with its pressure value opened for one minute.
Objective The objective of the experiment was to measure and analyze the reaction rate of tert-butyl chloride with sodium hydroxide, and plot it in a graph in order to observe the rate. Procedure Part A- Measurement of the SN1 Reaction Rate of Tert-Butyl Chloride • 100 mL of a solution of propan-2-ol and water (1:1 ratio) were collected from a container provided by the instructor, and they were placed in a 250 mL Erlenmeyer flask, which was subsequently cork-stoppered. Afterwards, 150 mL of NaOH were acquired and placed in a beaker, and in turn this 150 mL sample of NaOH was used to fill a 50 mL buret to the highest mark, and this buret was attached to a butterfly clamp attached to a ring stand in preparation for a future step.
Hydrolysis Rates of Esters Purpose Esters can be hydrolyzed to the corresponding carboxylic acid and alcohol with a decrease in the pH level as the acidic component is formed. The purpose of this experiment is to compare the hydrolysis rates of esters by monitoring the pH values of their aqueous solutions as a function of time. The esters being compared are ethyl acetate, ethyl benzoate, ethyl formate, and ethyl butanoate while the pH level can be determined by the change in color of the solution with the use of sodium hydroxide (NaOH) for the base and the universal pH indicator. The two factors that affect the rates for the hydrolysis of esters is the steric factor and the electronic factor which will serve as the determining factor of how
The purpose of this experiment was to observe and conclude the impact of a higher alkalinity and increasing sodium chloride concentration had on the yield of lysozyme crystals through crystallization. The constants for this process were sodium acetate at a concertation 0.05 M for every well in both rows, along with the concentration of polyethylene glycol (PEG) being set at 10% for every well in both rows. The two rows of wells that were tested deviated in alkalinity, row A having a pH of 4.5 and row B having a pH of 4.8, along with the sodium chloride concentration of each well. The concentration was increased by 0.5 M each well following the control well of 0.0 M sodium chloride.
Abstract In this experiment, the reaction kinetics of the hydrolysis of t-butyl chloride, (CH3)3CCl, was studied. The experiment was to determine the rate constant of the reaction, as well as the effects of solvent composition on the rate of reaction. A 50/50 V/V isopropanol/water solvent mixture was prepared and 1cm3 of (CH3)3CCl was added. At specific instances, aliquots of the reaction mixture were withdrawn and quenched with acetone.
A total of 0,2mL from the water obtained from the rinsing was placed in the STV containing LAL reagent and was shaken for 20 to 30 seconds. Then STV was placed in an incubator at 37 ° C for 60 ± 2 minutes. STV was then observed by reversing the reaction tube in one smooth motion. Negative controls performed using pyrogen-free water that is poured into a glass beaker which has been
Abstract The purpose of the experiment was to test which antacid medicine was most effective in decreasing the acidity levels in the stomach. Titration experiments involving hydrochloric acid and sodium hydroxide were used to test different antacids to see which one needed the least amount of sodium hydroxide to turn the solution pink. The antacids that were being compared in this experiment were Alcalak, Alka-Seltzer and Medi-First. With the use of M1 x V1 = M2 x V2 the excess volume of hydrochloric acid was found in order to find the amount of hydrochloric acid volume neutralized out of the original 100 mL of hydrochloric acid.
Introduction: A calorie is a measurement of energy, specifically heat. Calories are vital to our bodies and are found in the food and drinks we consume. The human body requires this energy to operate and perform daily functions, because without it, our cells would die. The energy we consume (food) needs to be at least the same as the energy we use (physical activity, or daily functions).
In this graph the results is about what we expected, which is a big amount of heat given off. In observing the graph the distance between reaction 1 and reaction 2 shows the total amount of heat given off which is the combination of 1&2 in comparison to room temperature that the water was originally at. Through the experiment there was a lot of question as to if we were doing it right, were we swirling the solution around enough, did we open the top right so heat would not escape, did we collect the data at the right time? Now looking back I see that many of the things that our group did defiantly altered our data, making me question the reliability of the data we collected. The first reaction was CaCO3(s) + 2HCL(aq)------- CaCl2(aq) + H20(l) + CO2(g) and the second reaction that was given was Ca(OH)2(s) + 2HCl(aq)-------CaCl2(aq) + 2H2o(l) combined gave off about 57 degrees Celsius going into a system (Calomitery and Hess’s Law).
Abstract: This Extended Experimental Investigation assessed the effects of the chloride salts; Lithium Chloride, Sodium Chloride and Potassium Chloride on levels of dissolved oxygen in samples of distilled water. The three salts and a control solution of pure distilled water were titrated thrice, each using the Winkler method, to determine the quantity of dissolved oxygen within the samples. It was expected that the saline solutions would have decreased dissolved oxygen content and that the larger the salt’s cation, the more oxygen would remain in the solution. The results portrayed that an increase in salinity, does decrease the levels of dissolved oxygen in water, however the results displayed that the larger the dissolved cation, the less dissolved
