The following materials will be gathered, a Coke Can Calorimeter, graduated cylinder, thermometer, ring stand, balance, a long thin stick, paper clip, matches, a marshmallow, a CHEEZ-IT, a Chex-Mix, and Cheetos. A Coke Can Calorimeter with a stick through the tab will be placed on the ring stand. An unwound paper clip will be placed directly underneath the calorimeter on the base of the ring stand. Water and a thermometer will be placed inside the calorimeter. The sample will be placed on the paper clip, so that the sample will almost be touching the bottom of the calorimeter. A match will be lit, and then will be used to catch the bottom of the sample on fire. A close eye will be kept on the thermometer to see when the temperature reaches
If there is an additional unmeasured amount of water in the Erlenmeyer flask, then this would reduce the concentration of the HCl, and therefore reduce the molarity. The volume of the amount of HCl solution added would increase, yet the concentration of the HCl would remain the same, which would ultimately result in the molarity of the HCl being lower than in reality.
1. 100 + 273 K = 373 K 150 + 273 K = 423 K 960 L x 423 K / 373 K = 1,089 L 2.
2) Heat one to about 50˚C, and place other one in calorimeter (at around 20˚C)
Use approximately 2 feet of aluminum foil to wrap around the burner stand and beaker to minimize heat loss.
Materials Used • Vernier LabQuest Temperture Probe • Ring Stand • Multiple clean, empty, 12-ounce soda cans with tabs • Water • Matches • Milligram Scale • Stirring Rod • Watch Glass • Timer • Various snack foods (Cheetos Puffs, Doritos, Potato Chips, Corn Chips) Safety considerations- Always tie long hair back, wear an apron and goggles at all times, be careful around matches- always blow the match out if the food does not ignite and the flame is encroaching on your fingers, be careful around the soda tab as soda tabs can cut open fingers, do not ignite the food near any other flammable objects that have a risk of burning, do not eat any of the leftover foods that was out in the lab- labs might have chemical residue that is not meant to be consumed, do not get super close to the
Our task was to identify the powder in each bag containing different amounts of moles. The mole provides a standard unit of measure that can be used to compare a wide variety of substances. A mole of atoms gives you a physical representation of what a single atom. The molar mass is the total mass of an element divided by one mole in that element. The molar mass can be used as a physical property to identify unknowns by converting it to moles and seeing which one is the closest to the moles in the bag. Our guiding question to answer was: “What are the identities of the unknown compounds?”
The materials we used for this experiment were two aluminum soda cans, water, ice, a graduated cylinder, a metal saucepan, a hot plate, and a
My hypothesis heading into this experiment was that the closer the flame was to the aluminum can, the higher the temperature/heat would be. This concept is pretty self-explanatory because fires are very hot and so if you put any object near a flame, the object will start to heat up. Setting up/completing this lab
We did our experiment using popcorn and bread. First we measured the mass of the pieces of bread and popcorn and we weighed their mass. We added 10cm of water into a test tube, measured the temperature. We heat the water with the help of the fire that caught on the food substance and we measured the temperature at the end when the food had completely burnt out. To find the energy released we used the formula, energy released = mass of water (g)*temperature rise *4.2/ mass of food sample (g)
Results from the experiment showed mass specific metabolic rate to increased as temperature decreased. An increased in metabolic rate is a result of an increased in respiration rate required from the mice to maintain internal body temperature at 37℃. Therefore, the hypothesis was supported because experimental data revealed respiration rate to increased as environmental temperature decreased. Experimental results can be supported by several published primary literatures that showed how environmental temperature affected an organism’s metabolic rate.
Calorimetry is the science of measuring the change in heat absorbed or released during a chemical reaction. The change in heat can tell us if the reaction is either exothermic - it released or heat into surroundings, or endothermic - it absorbed heat from surroundings. The device used to measure calorimetry is a calorimeter. A calorimeter can range from very expensive lab ones to coffee styrofoam cups but they are all tightly sealed in order to prevent heat from escaping.
The molar mass of unknown one at 0.2252 g is 248.29 g/mol, at 0.2252 g it is 248.29 g/mol, and at 0.2482 g, it is 91.25 g/mol. The average molar mass calculated is 205.07 g/mol. There was a jump in the molar mass value at different weight. This could have been due to the experimental errors that occurred during the lab. The graph of the solvent solution initially begins at 23.8˚C but jump down to 10.5˚C. This makes a huge impact on the results of the data because the freezing point should start earlier in time than it shows in the data sheet.
The heat of combustion produced increases the temperature of the calorimeter system. About 10 to 15 minutes after ignition the heat exchange between the calorimeter bomb and the water surrounding it in the inner vessel is completed. The temperature rise is then measured and serves to calculate the gross calorific value Ho. This calculation is possible only if under the same test conditions the heat capacity C of the adiabatic system has been determined previously by burning a reference
Use the test tube holder and hold one of the tubes at a 45° angle. Gently heat its contents over the burner, slowly passing it in and out of the flame. Record any change in the appearance of the compound.
As for the part two the experiment, the class was divided into two groups and both groups were specifically assigned to determine ΔS and ΔH. In order to determine ΔS and ΔH, the calorimeter apparatus was set up first. After, the materials that were also needed was the igniter and the fuel. The lab coordinator provided the groups with those materials. The igniter was initially weighted and was determined to be 0.057g. After, the initial weight of the igniter was recorded, it was then inserted to bottom of the fuel. Then the combination of the igniter and the fuel before the combustion was weighed, which was 0.647g. The igniter