“Ice…Ice…Baby” “What is the quickest way to melt ice?” January 22, 2013 Abstract We choose to do this experiment in an attempt to discover what the quickest method for melting ice was. The purpose of this project was to find a way to melt the ice off the glass of a car windshield during the cold winter months. Our hypothesis was; if we added water to the ice it would melt quicker then adding either air or salt. The independent variable of the experiment was the molecular structure of the water found in the form of an ice cube. The dependent variable was the “amount” of time it took for all 3-ice cubes to melt.
Rate of reaction IA Temperature vs. Rate of Reaction Experiment to investigate the effect that temperature has on the rate of reaction. Objective: In this experiment Iodine and Starch solution will be mixed together at various temperatures in order to determine the effect that temperature will have on the rate that the reaction will occur at. Materials: * Starch Solution x 1 * Iodine Solution x 1 * Thermometer x 1 * Ice placed in beaker x1 * Beakers (250cm3) x 3 * Large beaker x 1 * Stopwatch x 1 * Bunsen Burner x 1 * Test-tubes x 6 * Empty Beaker x 1 * Matches x 1 * Notebook x 1 * Pencil x 1 Safety and environmental care: * Avoid direct contact with any hot objects, ensure that clothing does not come into contact with flame. * Safety glasses are to be worn at all times whilst the experiment is in motion. * Gloves are to be worn whilst the experiment is in motion.
Determination of Freezing Point and Verification of Freezing Point Depression for a Mixture by Linah Richer Partners: Maike Blakely CHM317 Preformed: Nov. 8th, 2013 Report: Nov. 19th, 2013 Abstract: The purpose of this experiment is to determine the freezing point of the solvent, biphenyl, and verify the freezing point depression equation ΔTf=-ikfnsolutemsolvent. The addition of solute will lower the vapor pressure of the solvent/solute mixture resulting in the lowering of the freezing point for the mixture solution. The experiment resulted in the experimental difference in the two trial freezing points to be 0.08 K leading to a calculated change in temperature freezing to be -1.92 E -5 K, and an overall decrease in temperature freezing of the solute/solvent solution compared to the pure solvent solution. Introduction: Experimentally it is understood that the addition of a nonvolatile solute to a solvent will lower the vapor pressure, raise the boiling point and lower the freezing point. In this experiment, the freezing point for the solvent biphenyl will be determined theoretically and experimentally, as well as the verification of the freezing point depression equation for a solvent/solute mixture.
Variable : Control - Water, 1000cc Independent - Dry ice amount, 1-10 Dependent - Temperature Background Information: Dry ice is frozen carbon dioxide, Co2, which can make lots of fascinating experiment. The temperature is around -109.3°F or -78.5°C. Which is good for keeping things cold, for example to keep box of ice cream cold. Dry ice is sublime faster in water rather than air. It was because the water transfers heat much more quickly to the surrounding.
Three tests will then be performed to examine the identity and purity of the synthesized aspirin. The first test will detect the presence of leftover salicylic acid in the synthesized aspirin. The second test uses melting point to evaluate the purity of the aspirin product. A compound that contains impurities will tend to melt over a range of temperatures and at temperatures lower than the fixed mp for the pure compound. The third test will utilize thin layer chromatography to evaluate the purity of the aspirin as well as testing for the presence of leftover salicylic acid or other by products of the reactions.
Introduction In Chemistry 1211 lab the main objective was to identify the name of the unknown acid #2651145-PLF13 that was issued by the instructor. Melting point, titration of the unknown acid, calculation of equivalent weight, pKa, solubility tests, and properties of a hydrochloric acid; these procedures were used to characterize the unknown acid and then compared with known substances using GSU Chemistry department search engine. By doing this experiment he or she will develop an understanding of the properties of organic acids and differences between properties of a strong acid such hydrochloric acid. Experimental The first procedure to identify the unknown organic acid was finding the correct melting point. This was done by taking small amounts of the unknown acid.
The effectiveness of lipase on temperature Abstract Enzymes are biological catalyst that speeds up the rate of reaction. Different enzymes work best at different temperatures, which is also called an optimum temperature. Different enzymes also have different functions. Lipases are enzymes, needed to break down lipids (fats and oils) into the products - glycerol and fatty acids. They work best at room temperature around 36-40 C. Introduction For this experiment, I will be looking at how the change in temperature affects the rate of reaction.
The Latent Heat Of Fusion Of Ice Lab Report In this lab , I chose a variable and investigated the effect of varying it on the specific latent heat of fusion of ice . Materials: * Electric Immersion heater * Funnel * Glass beaker * An ammeter * A voltmeter * Power supply * Stopwatch * Retort stand & clamp * Ice * Mass balance Hypothesis : Simply, If time changes it won't change the latent heat of fusion in ice. Used Equations: Energy in Joules = Voltage x Current x time (s) Latent heat = Energy (joules) / mass (kg) Procedure : 1-Set up the apparatus as shown in the diagram but without the ice . 2-weigh you beaker. 3-Crush the ice and put it in the funnel trying to pack it closely round the heater .
3. Evaluate the hypothesis and the procedure performed. Hypothesis: If the mass of the metal is greater, then the temperature change of the water will increase. Safety: Glasses must be worn, and loose clothing restrained for the Lab Exercise! Materials: 250mL Beaker Test Tube Calorimeter Burner, Ring Stand, and Wire Gauze Thermometer Balance Procedure: 1.
Experiment 15: Molar Mass Determination by Freezing Point Depression Introduction The purpose of this experiment is to determine the molar mass of camphor by determining the freezing point depression of cyclohexane. In this experiment a sample of the solvent cyclohexane was cooled to its freezing point and a cooling curve was constructed. A known mass of camphor was added to the known mass of camphor and the freezing point of the solution was determined using equations 1 and 2. From the freezing point depression the molality of the camphor can be calculated and then the molar mass, by using equation 3. If Tf(solvent) is defined as the freezing point of the pure solvent, and if Tf(solution) is defined as the freezing point of the solution, then the freezing point depression (in °C) is given by equation 1: ΔTf = Tf(solvent) - Tf(solution) (1) The freezing point depression ΔTf is related to m, the molality of the solution particles, given in equation 2: ΔTf = Kf m (2) If a known mass of a solute is placed into a known mass of solvent, and the freezing point depression relative to the pure solvent determined, then the molar mass (MM) of the solute can be determined by using the appropriate Kf value for the solvent, equation 3: ΔTf = Kf (mol/kg solvent) = Kf (g solute/MM solute) / kg solvent (3) Procedure Determination of the Freezing Point of Cyclohexane A 20 x 50 mm test tube was rinsed clean with cyclohexane.