Our objective was to pick the best chemical to be used in a hand warm. This chemical had to be cheap, relatively safe, and must raise the temperature by 20oC and no more. We add 6 different chemicals to water we record the inshell temperature and then add one a the 6 chemicals to the water and record the temperature change of the water. We also add cold water hot water together to find how much heat would escape the calorimeter. We found that the calorimeter absorbed 71.1J/oC. Then this information to calculate the energy that was released by all of the chemical reaction. We found that Joules from NaCl = 340 J, NH4NO3 = 1340 J, CaCl2 = -2320 J, LiCl = -3600, Na2Cl3 = -720 J, NaC2H3O2= 1070 J. Then we used energy release from one one these rxn to calculate the Hor the KJ per mol rxn.
The following procedure was taken from the 2017 Millsaps College lab manual.1 The experiment was split into two parts, part A and part B. Part A was to find the heat capacity while part B determined the specific heat of an unknown metal. This was the final goal of the lab. To start, a temperature probe had to be connected to a LabQuest2 data collection device. 100.0 mL of deionized had to be added into a Styrofoam cup. The temperature probe was kept in the calorimeter until the temperature had been stabilized and was calibrated. A beaker was placed on a hot plate with dial turned between three and four. Another 100.00 ml of deionized water was added while the beaker is heating up. Using the temperature probe, the beaker was measured
The average experimental mass was 144.5 grams per mole as shown in Figure 6, which is a 20% error from the accepted molar mass of glucose 180.16 grams per mole as is shown in Figure 7. Errors could have come from the ice bath not being cold enough, not all the powder transferred into the 11 dram vial, and not dissolving all of the powder. The usage of tap water instead of distilled water would have affected the results for tap water contains other ions which would then affected the freezing point depression. Salting icy roads and walkways lowers the freezing point of the water that forms ice which leads to melting and prevents falling snow or rain from being able to freeze.
The ability to carry out metabolic processes, or the chemical activity that occurs in all living organisms, is essential to maintaining life. The total metabolism of an organism is made up of anabolic and catabolic pathways. Anabolic pathways expend energy to build important molecules. On the other hand, catabolic pathways release energy to break down important molecules. The energy found in in these pathways is from respiration. Respiration is the process by which organisms consume oxygen to create energy. By measuring oxygen consumption, the metabolic rate can be determined because of its correlation to respiration. In this experiment, the rate of oxygen consumption is measured in water using the poikilotherm goldfish. Unlike the body temperature
Background: Calorimetry is the science of measuring heat based on observing the change of temperature when a body takes in or gives off energy as heat or light. The device used to determine heat associated with a chemical reaction is called a calorimeter. When calorimetry is used it’s information is then put into an equation to find the specific heat of an object. The equation is, SMΔTwater=SMΔTobject. This means that the specific heat times the mass and change in temperature of water will equal the specific heat times the mass and change in temperature of the object.
Introduction: By now, you are aware that scientists apply heat to substances in order to decompose them. In this lab, you will apply heat to make copper sulfate pentahydrate (CuSO4●5H2O) undergo a decomposition reaction. You will make observations and will have to make an educated claim about the products of the decomposition reaction. Furthermore, you will have to use your observations as evidence and will have to discuss your reasoning about why your observations support your claim.
In this lab we separated a mixture to observe the methods of separating substances from one another using a series of techniques. In this lab we used magnetism, filtration, and evaporation to successfully separate the mixture into three separate components. Throughout the experiment we learned that mixtures are two or more substances combine and each substance retains its own properties and chemical identity.
The variable being manipulated is the reaction between 2 g of solid copper (II) sulfate pentahydrate and 2 mL of 6 molar hydrochloric acid with approximately .25 g of aluminum foil being conducted in a real lab in addition to theoretically on paper, where the reactants are expected to create the product of an acidic, aqueous solution of copper (II) sulfate pentahydrate.
The experiment began by setting up the LabQuest and preparing a 2M solution of HCl and a 2M solution of NaOH. This was called “Part A”. Two general rules were noted throughout the experiment: add acid to water and pour stock solution into beaker before graduated cylinder. This prevented flash-boiling of the solution, chemical burns, and spills. To make the 2M HCl solution, 200mL deionized water was added to a 600mL beaker labelled “2M HCl” by using a graduated cylinder. Then, 100mL 6M HCl was added to the same beaker also by using a graduated cylinder. The solution was stirred with a stirring rod. To make the 2M NaOH solution, 50mL deionized water was added to a 400mL beaker labelled “2M NaOH”. Then, 100mL 3M NaOH was added to the same beaker.
Freezing point depression is a colligative property that calculates the decrease of the freezing point when any solute is added to a solvent. When determining changes in freezing point, solute concentration is measured in molality which is moles of solute per kilogram of solvent. The concentration unit moles per kilogram is temperature independent, because mass does not vary with temperature. The decrease in freezing point of the pure solvent is proportional to the molality of the particles of solute and is represented by the following equation: ΔTf=Kf ۰ m. By finding the freezing point of an unknown solution, it provides an opportunity to determine the molar mass of the unknown substance. Also, in this experiment a heating