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Report in carrying out calorimeter experiment
Chemistry reactions and observations lab
Calorimeter lab report
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Recommended: Report in carrying out calorimeter experiment
A hot plate was placed under the ring stand. 50 mL of 3.0 M NaOH in a 250 mL beaker and a stir bar was placed in the beaker. The beaker with NaOH was placed on the hot plate and 3.75 grams of NaAlO2*5H2O was placed in the beaker. The temperature probe was placed in the beaker with the solution, not touching the bottom of the beaker. The solution was heated and stirred till the solution dissolved.
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.
The converse was true for the 5% NaCl solution without Elodea and the 5% solution with Elodea (table 1). A comparative observation revealed that the beaker with Elodea in salt solution required more NaOH than did the beaker with Elodea in tap water (figure 1). Table 1. The number of drops of NaOH in each beaker Beaker Name Number of Drops Tap Water
The purpose of this experiment was to use a pH meter to graphically determine a stoichiometric point, to determine the molar concentration of a weak acid solution and the molar mass of a solid weak acid, and to determine the pKa of a weak acid. In part A of the experiment, the unknown named Luke Skywalker was used during the experiment. Throughout the experiment the experimenter collected measurements such as the number of moles of NaOH to stoichiometric point (0.00115 mol, 0.00105 mol) and the molar concentration of the unknown acid (0.046 M, 0.042 M) during part A of the experiment. During Part B of the experiment the experimenter collected buret readings of NaOH and determined the stoichiometric point and volume of NaOH dispensed. Based
The purpose of the “Titration of the Unknown Acid” lab is to determine how much of a given material known as concentration is in a substance or mixture. In this lab, the student also learns the technique of using titration. The concentration of the acid we used in class will be sampled with a standardize solution such as sodium hydroxide with an environmentally indicator to show the physical change of color that occurs to the solution by the acid. The equipment necessary for the titration experiment follows: 0.1M NaOH, Acid solution, Anthocyanin (which is found in red cabbage leaves) indicator, Burets, Ethanol 95% and DI water. First Professor Greenberg assign a labeled unknown acid solution, then we recorded the solution’s identity and bottle code.
At the start of the experiment, an unknown acid, the solute, was dissolved in DI water, the solvent, diluting the concentration of the acid. Phenolphthalein, an acid-base indicator--or a weak acid that changes color when the equivalence point is reached--was added to the solution. The solution was then titrated, a process by which a solution with a known concentration, NaOH, is added to an unknown solution, the acid, in order to determine its concentration. The reaction consisted of an unknown weak acid and NaOH, a strong base, making the reaction a weak acid-strong base reaction. Because NaOH is a strong base, the pH of the reaction--or the measure of the acidity of the solution by taking the negative log base ten of the hydronium concentration--would increase when titrating the unknown acid.
The experiment for this report is 5, 6, and 7. In experiment 5 there are given a Sodium Hydroxide which is 4.126 g when it is weighted and a KHP also with the NaOH there’s two other experiment that are used to find the titration of molarity in the three chemical balances. In exp. 6 and 7 there using the NaOH to find titration in an acid and vinegar by going through three trails to see how much sodium hydroxide is pick in it until it turns light pink, however if it turns dark pink there’s an error in the trail.
The Calorimetry experiment is the use of a calorimeter to measure a temperature change. Calorimetry is the measurement of heat.1 This can later be used during calculations to find the enthalpy of an equation. Essential to calorimetry is the calorimeter, which can be any device for accurately measuring the temperature of a substance before and after a change occurs.2 A calorimeter can be as simple as a styrofoam cup. Its quality as an insulator, which makes styrofoam ideal for holding in the warmth of coffee and protecting the hand from scalding as well, also makes styrofoam an excellent material for calorimetric testing.2 The first law of thermodynamics is energy cannot be created nor destroyed but it can be transformed into another type or be transferred into another object.3 This is important to understand because during calculations it would allow one to understand why one would have to calculate the amount of heat transferred to the calorimeter.
Based on the R2 values from your graphs, do you think that density trends on the periodic table are linear relationships? What rationale could you offer to explain your answer? The R2 value established from the group 4 graph demonstrates a linear relationship with a steady increase. The period IV graph provided a very low value of R² = 0.0028 on the linear trendline and presents nearly any correlation at all.
Procedure: Put on goggles and apron. Get unknown metal block. Measure the weight of the block in grams using a scale.
In this experiment, each of the unknown solutions were tested for the presence of chloride, nitrate, and acetate. For unknown 2, there was no precipitate formed during the chloride test, concluding that it did not contain chloride. Unknown 2 also produced a negative for the nitrate test, since a brown ring did not form, indicating that it did not contain any nitrate ions. The last test, the acetate test, was not conducted on unknown 2 due to the results from the cation tests. For unknown 4, the chloride test also produced a negative result, indicating the absence of any chloride ions.
The equation of the reaction between sodium hydroxide and ethanoic acid is as follows: CH3COOH + NaOH → CH3COONa + H2O We can measure the end point of titration process and we can also measure the amount of reactants. The concentration of ethanoic acid in the vinegar can be determined through stoichiometric calculations, Using the values obtained from the titration, and also the chemical equation as a reference. Phenolphthalein indicator is used in this acid-base titration Equipment and materials:
Title: 3.5 Thermal Radiation Date Experiment was performed: 23/2/2018 Lab Partners Name: Dylan Loughnane (15152642) Mark Timlin (14165457) Author of Report: Rebecca Gavin (16153111) Name of Module: Thermal Physics (PH4042) Aims: In this experiment we're trying to show how heat transfer is a mechanism of conduction, convection and radiation. We do this with a two part investigations. First part of the lab will test the stefan-boltzmann constant at high/low temperatures and how different temperatures.
The Calorimeter Calorimetry is the science that was first recognized by a Scottish physician and the scientist Joseph Black. It is related with determining the variation in energy of a system by measuring the heat transfer with the surrounding. It is derived from the word calor in Latin, which means the heat and the pressure. Calorimeter is the device used in the calorimetry science to measure the quantity of heat transported from or to an object. Heat is the transfer of thermal energy between two bodies that differs in temperature (Mc Graw Hill Education).
That caused a new initial reading of NaOH on the burette (see Table1 & 2). The drops were caused because the burette was not tightened enough at the bottom to avoid it from being hard to release the basic solution for titrating the acid. The volume of the acid used for each titration was 25ml. The volume of the solution was then calculated by subtracting the initial volume from the final volume. We then calculated the average volume at each temperature.
