Tin Foil Lab Report

In this experiment, two Styrofoam cups and a brand calorimeter are each used to calculate heat transfer. The results will be compared to see if the something as simple as a Styrofoam cup can be used accurately as a calorimeter and produce efficient results. Using hot and cold water, the Styrofoam cup and brand calorimeter will be used to determine the heat capacity. By using the mass of the water, specific heat of water and the change in temperature, the heat capacity will be determined. The brand calorimeter and Styrofoam calorimeter

Prior to starting the experiment, to keep the water temperature stable and consistent, the proposal to ensure this would happen was to utilise the water baths. Due to the shortage in equipment, the method was then amended to use two plastic containers and use a kettle to ensure that the water temperature was consistent. This was to guarantee that the results collated were accurate for all trials conducted.

The mole is a convenient unit for analyzing chemical reactions. Avogadro’s number is equal to the mole. The mass of a mole of any compound or element is the mass in grams that corresponds to the molecular formula, also known as the atomic mass. In this experiment, you will observe the reaction of iron nails with a solution of copper (II) chloride and determine the number of moles involved in the reaction. You will determine the number of moles of copper produced in the reaction of iron and copper (II) chloride, determine the number of moles of iron used up in the reaction of iron and copper (II) chloride, determine the ratio of moles of iron to moles of copper, and determine the number of atoms and formula units involved in

Introduction: Yeast (saccharomyces) is a common single-celled fungus. They are microscopic plants that exist naturally on Earth. They are known for their ability to ferment the carbohydrates in the flour and gain energy from this digestion. Some food products created by yeast include bread, beer, wine and cheese. Yeast is mistaken as lifeless, dry powder used to make bread, but, it becomes active in moist environments.

Using a piece of aluminum foil with a slit in it, place the foil between the base of the flame and the liquid in the bowl. Note the behavior of the flame. 7. Invert a beaker over the lit flame. Make observations

October 17, 18, and 19, samples were collected from multiple sites along the BSR. The class was split into groups, and samples were collected from seven separate locations along the river and WWTP. There was also a sample collected by the S which is located between sites four and five. For each of these sites, there were ten groups from other labs that also collected a sample from the BSR. At site two of the river, the location included multiple sources of possible contamination. A drainage site was located 200 yards upstream, along with a small PVC drainage pipe next to the collection site. Not only was there drainage running into the river, the site was under a bridge, and contained other trash scattered throughout the area. The

50mL of 2M NaOH was added to the two stacked Styrofoam cups in a 400mL beaker. The cup was then covered with a plastic lid and a temperature probe was inserted through the lid and into cup in a way so that it did not touch the bottom. 3-4 temperature readings were then collected by clicking “collect” on LabQuest to start Run 2, and initial temperature was determined. 50mL of 2M NH4Cl was then added to the NaOH solution in the cup and swirled around. The rest was repeated from the first

Sugar in Coke Lab Report Sheet: Raghed Odeh 10/18/2017 Provide a brief statement of the purpose of this activity and explain the idea behind a calibration curve (this can be done before class and valuable insight can be gained by watching the “weblets” (online prelab lectures available in the course content of D2L). The purpose of this lab is to determine the amount of sugar (in grams) in a can of coke, learn how to make solutions quantitatively and learn how to make and use a calibration curve. A calibration curve is used to understand the instrumental response to an analyte and predict the concentration in an unknown sample. As long as a function is known, the curve can be made.

The goal of this specific study is too attempted to get a constant temperature change throughout the experiment. (insert ANY TERMS USED). This study would be related to the second law of thermodynamics, across the board if planned and executed right each time we mixed the corn syrup and the water together we should have got the same thing out of it. 1)Gather your supplies. The supplies being Corn syrup, Water, Graduated cylinder, Beaker, Gloves, Hot plate, lab quest and a pair of goggles.

For the first trial 100 mL of distilled water was poured into a 500 mL beaker and placed on a hotplate to warm to 40 °C. While waiting for the distilled water to warm to the desired temperature, two sponge animals both red and blue were selected and weighed on the scale for their beginning weight individually. After some time elapsed, the water temperature was measured with a stirrer thermometer, which was observed to never touch the bottom of the glass beaker. After the water was warmed to the desired temperature, 50 mL of the water was poured into a graduated cylinder, and then poured into the Styrofoam cup. The remaining liquid was then poured into the graduated cylinder, and then poured into the remaining Styrofoam cup.

Insert a thermometer, and measure the temperature of the contents to the nearest tenth; place the foam cup and its contents on the electronic balance

Our thermos was quite effective in insulating hot water, as the graph was very flat. This indicates that as time passed, the temperature of the hot water dropped very little, resembling an exponential decay graph. Trial one and trial two presented very similar results and a constant rate of change, which further reinforces the effectiveness of the thermos. The second trial basically presented identical data to the first trial, which can be seen on the graph as the two lines are merged together. The lumps in the graph for the control were resulted from the accidental moving of the temperature probe or the occasionally currents of air flowing across the cup,

2) Although, the copper calorimeter was properly insulated, heat loss was prevalent. The lid had a

Place the plastic bottle with water under the heat lamp with 100 watts of incandescent light bulb turned on

There will be glass and boiling water in this experiment. For safety reasons, ONLY the instructor may pour the boiling water into its container. The container MUST be held with the thick towel provided by the instructor. If any glass is broke, inform the instructor immediately.