Darryl And Faith's Thermal Mass Temperature Experiment

The aim of the experiment was to find out how changing the mass effects the rise of the temperature of water.

In this lab, there are two days. In the first day, there are is part A and part B. Part A is further divided into three experiments. In experiment one, we were to figure out the heat capacity of the calorimeter that we made. The next two experiment’s goal was to calculate the enthalpy of 2 reactions and using hess’s law, figure out the heat of formation of magnesium oxide. In a reaction, there are

Each student got a white tub and filled it up with tap water from the sink. Students were paired with two or three other people and formed their groups. Each group got 1 stopwatch, 1 thermometer, and also learned how to each other’s pulse. The temperature of the water used from the sink were adjusted beforehand to about 23°C; room temperature. Water temperature was not re-adjusted to be hotter or colder.

Again with the same temperatures of one degree, eleven degrees, twenty degrees, thirty degrees, and forty degrees. All the temperatures are in Celsius. The one degree C time is at 24.59 seconds, only two seconds off from the first trial. The eleven degrees C time has 20.39 seconds. At twenty degrees C, the data showed the time was 15.54 seconds. Thirty degrees C had the lowest time of the thirty degrees group, at 8.97. The last temperature was forty degrees C with the lowest time at 7.28 (See appendix two). All the data for trial two supports the hypothesis for this

A scale conversion is calculated and the measurements from each thermometer are examined to see how closely correlated they are. _M___

The percent mass of each component of the mixture was 23% iron, 61% sand, and 8.7% salt.

The boiling point elevation constant for water that was experimentally determined in this analysis was 0.4396 °C/m, which was derived from the slope of the trend line in Figure 2. This is slightly lower than the constant provided in lecture of 0.51 °C/m. This could be due to further evaporation of water from the solutions tested via refractive index after the boiling temperature was recorded.

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.

In this experiment, a mixture of unknown #3 was used. That mixture had acid, base, and neutral. We added solvent to the unknown. It is important to know the density of the solvent in order to determine which is the aqueous layer and which is the organic layer. If the solvent that has more density than water, so the organic layer will be the lower layer, while if the solvent has lower density than water, the organic layer will be the upper layer. This will make an error if the determination of the layers was wrong after added the strong acid or the strong base. We added 5% HCl to the mixture in order to separate the base in the aqueous layer and form its salt. Same thing, we add 5% NaOH to the mixture in order to separate the acid and form its salt. In order to recover the base, we add 10% NaOH to the HCl extraction. The result will be salt with a base. Same thing for the acid, in order to recovered it, we added 10% HCl. The reaction will give us salt with an acid. For the neutral, we added sodium sulfate as a drying reagent in order to dry water and separate the neutral part as pure.

1. In the human blood, there is the bicarbonate buffer system. CO2 is released from cellular respiration and then taken up by red blood cells. Next, it is changed to carbonic acid which dissociates to form bicarbonate and H+ ions.

The main purpose of the lab “Determination of the Formula of a Copper Oxide” was to determine the formula of a copper oxide. Specifically, this is a compound of copper combined with oxygen. This was to be done by heating the copper oxide thoroughly until all of the oxygen had been driven off. To accomplish this experiment, we first had to take and measure the mass of a specified color of copper oxide, ours being red. Then, we used a fischer burner to provide the heat needed for the split of copper oxide, in which our amount resided in a test tube. But, in order for the copper to not recombine with oxygen that could be found in the surrounding atmosphere of our lab, we also had to have a flow of methane gas into the test tube that fed into

The initial magnesium had a mass of 0.06 g while the final compound had a mass of 0.08 g. Magnesium oxide had been formed, and no magnesium should have been lost over the process due to magnesium being unable to form gases or liquids with any of the elements it had been exposed to.

2. Some of the outside variables that could have affected our outcomes for the experiment are the ambient temperature and how quickly the groups took the hot dogs out of the ice water to measure their temperatures. The ambient temperature was 28 degrees Celsius, the coldest temperatures of the hot dogs ranged from 35 to 37 degrees Celsius, so for the groups that measured their hot dogs’ temperature quicker, they gave their hot dogs a head start in the warming process. For groups that were not as quick with their measurements, their hot dogs starting warming up at a later time, so by the time the experiment was over, their temperatures would have been lower than the groups that measured quickly. We did not control these outside variables because we did not increase or decrease the room temperature by turning on the AC.

The initial circumference of the balloons were 41.5cm. The temperature of the hot water was 58℃, the room temperature water was 25℃ and the cold water was -4℃. After the balloons were placed in the water for 3 minutes, we got our results. The final circumference of the balloon in the hot water was 40.5. It shrank 1cm less which is a surprise since it should expand.

The purpose of Step 8 is to make sure we get the exact mass of the solution. There could be trapped molecules of water in the solution. Heating the solution would evaporate the water molecules.