Beaker Temperature Lab Report

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

Why does the Alaskan Way Viaduct Collapse? The Alaskan Way Viaduct hasn’t really collapsed yet. Even though it hasn’t collapsed yet we know what is going to cause it. It all starts with the layers of the Earth.

The lab started off by measuring critical materials for the lab: the mass of an an empty 100 mL beaker, mass of beaker and copper chloride together(52.30 g), and the mass of three iron nails(2.73 g). The goal of this experiment is to determine the number of moles of copper and iron that would be produced in the reaction of iron and copper(II) chloride, the ratio of moles of iron to moles of copper, and the percent yield of copper produced. 2.00 grams of copper(II) chloride was added in the beaker to mix with 15 mL of distilled water. Then, three dry nails are placed in the copper(II) chloride solution for approximately 25 minutes. The three nails have to be scraped clean by sandpaper to make the surface of the nail shiny; if the nails are not clean, then some unknown substances might accidentally mix into the reaction and cause variations of the result.

In actual fact though, you may not even know that the error exists. Some systematic error that occurred in this was density depends on temperature. The temperature was not specified or controlled. Random errors are chances in variation in the measurement over which you as experimenter have little or no control. Some errors were slight variations in the level of your eye while reading the meniscus in the graduated cylinder vibration in the floor or air currents that cause fluctuation in the

2) The glass beaker was placed in the freezer. 3) The temperature of the heavy whipping cream was checked with the thermometer every few minutes until its temperature reached 3˚C. 4) The heavy whipping cream, which was then at 3˚C, was transferred from the beaker to the container.

50mL HCl was added to the calorimeter, which was covered with the lid and inserted with a probe. Readings were collected and then 50mL NH4OH was swiftly added to the solution, with the stir bar mixing the reaction constantly. The initial and max temperature temperatures were recorded and the change in temperature was recorded. The data was saved onto the USB.

As mentioned in the hypothesis, the prediction is that as the temperature increases towards the optimal, the rate of respiration will increase. As the temperature exceeds the optimal, the rate of respiration will decrease. The temperature of the environment can be varied by placing the respiration chamber under a temperature-controlled water bath/cooling bath. The temperatures that will be used in this experiment will range from 0ºC to 50ºC in 10ºC increments. Digital thermometer will be used to measure the temperature of air.

“Collect” was clicked to begin data collection. Once the pressure and temperature stabilized in the boiling water bath, “Keep” was clicked. The heating was turned OFF on the hotplate, and ice was added to the bath to cool it. “Keep” was clicked once the temperature of the bath cooled to 95°C. The procedure was continued as the temperature continued to decrease, and “Keep” was clicked at every 5°C increment until the bath reached 0°C.

They tested how the temperature would affect the rate of reaction. This was observed by the amount of time it took for the solution to change colors. For many chemical reactions there is an optimum temperature at which the chemicals will react with each other. As was found in their experiment, the temperature affected the rate of reaction. (Deoudes, 2010).

Using the data from the first two columns, an x-y scatterplot graph was created. Analyzing the graph, a set of points that formed a linear curve were identified, and the plot of the graph was reduced to these points. This is the initial cooling curve. A second series was then added to the graph, with points that correspond to the interval when t-butyl alcohol was freezing. A trendline was then created for each of the series to obtain the equation of the line and r values.

Materials: The materials that I will be utilizing during these experimentations are three to four ice cubes, one cup for measuring, six unblemished cups, one stopwatch, one hot water source, three tablets of Alka-Seltzer, one thermometer that measures from negative

37.8 °C and 36.3 °C 30-40 °C 3. 41.7 °C and 40.2 ° C 40-50 °C 4. 50 °C and 48 ° C 50-60 °C Average temperatures: (37.8+36.3)/2=37.05 °C (41.7+40.2)/2=40.95 °C (50+48)/2=49 °C Table 1 -The values of experiment Temperature (°C) Density (kg/m3) 26.5 995 37.05 992.5 40.95 991 49 990 70 984.856 80 982.524 90 980.272 100 977.93 Table 2. The values in steam table Temperature (°C) Density (kg/m3)

Because of this, the experiment was done at constant temperature. If solutions 1-5 had been done at different temperatures, there would not have been a way to determine the effect of the change in temperature on the magnitude of the equilibrium constant. In order to be able to determine the magnitude, the original K value would first need to be determined. Once determined and both temperatures were measured, an experiment could be done to determine the K of the second

Turn off the circulation for chiller 1 and turn on the circulation for chiller 2, and start sampling 11. Increase the temperature of chiller 2 to 12.5oC and keep it at the same temperature for 6 minutes OR alternatively, raise the initial chiller 2 temperature at a faster rate. 12. Keep raising the temperature at the rate of 0.5oC every 6 minutes until arrhythmia is reached and determine TArr. 13. As TArr is approached, stop and bring the temperature of the heart down to 5oC lower than TArr.

Place the the beaker onto a hot plate that is on a low heat setting (about setting 3). Every 5 minutes for 20 minutes, measure the circumference of the balloon and record it in Data Table A. You can measure the circumference of the balloon by looping a piece of string around it then using a ruler to measure the string’s length. Record the data in the data