Specific Heat Lab Report

This was concluded by simply comparing the initial and final temperatures of the substance(s) in the two plastic bags. Using prior knowledge, I knew that if there was a decrease in temperature, an endothermic reaction had taken place. But if there was an increase in temperature, an exothermic reaction had taken place. Comparing the two temperatures (I=23℃, F=17℃), a decrease in temperature was very noticeable. Based on the facts stated previously, an endothermic reaction had taken

We calculated the density of the metal ball to be 7.83 g/cm3 using methods IV and V and concluded it was iron. C. The density of the plate was calculated to be 2.667 g/cm3 using methods IV and V. Thus we concluded that it was aluminum. 3.

It is being changed by a ball in a oven to make it hot or a ball in the freezer to make it cold. Temperature can be measured by

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.

The science behind this is very simple, it involves the behavior of gases. Atoms in a gas is free flowing. They respond and move faster when there is heat, and slower when it is cooler because of a loss of energy. It then changes the pressure of the gas, as the atoms in a certain volume of gas changes. In this experiment, we heated to can with water in it until it was boiling, which

Utilize a test tube brace to put the test tube containing the obscure strong in the bubbling water shower. Warmth until the greater part of the strong melts. Pour 140-160 mL of faucet water into a 250-mL graduated barrel. Record the volume to the closest 1 mL. Place a buret clasp on a help stand. Gather a calorimeter.

4. Errors could occur in the graph if we don’t read the thermometer right and don 't write it down right, also you could graph it wrong and put something in the wrong place. You could also not be paying attention and miss 2 minutes or something and then the results wouldn 't be fair. Other errors that could happen could be knocking over the beaker, not using a protection mat or putting the wrong amount of water in the beaker before placing it in the

To control this, the water being used will be placed inside a room with a room temperature of 20°C for an hour to allow the temperature of the liquids to drop and remain at that temperature. Apparatus List: A wine glass. An electric thermometer to measure the temperature of the water.

Lastly, it told us to repeat the same steps until we had three calcium chloride scoops in the beaker and repeat for two more trials for accurate results. To sum up the experiment, it said to record the average change in temperatures to the class averages to graph a bar graph comparing both of the averages. That’s the procedure on how to conduct the experiment correctly. The averages that my group received for zero scoops were 0.5 degrees Celsius, one scoop was 6.5 degrees

Synopsis This laboratory report gives an outline of the experiment which was carried out in order to measure the density of water at different temperatures via two different methods. The lab consisted of two parts. In the first part the density of water was measured by hydrometer. At first the density of water at room temperature was measured.

This temperature made the soup that was used to boil. The soup used is a vegetable soup that was not that watery. Vegetable soup was chosen because it is easy to make and it was available during the experiment being performed. The reason why the temperature of the

This coil has an electrical resistor which resists the flow of electricity, which in effect converts electrical energy into heat as energy goes through the coil. Due to this, the heat energy produced by the resistor heats up the water within the kettle to boiling point. The heating element is controlled by a bimetallic thermostat, which contains a variable resistor inside it. Integrated at the bottom of the kettle, it consists of a disc of two different metals bonded tightly together, curved in a particular direction. As temperature inside the kettle rises, one metal expands faster than the other, set up in a manner

The point of the experiment was to test how accurate and precise five pieces of lab glassware--an erlenmeyer flask, a pipette, a buret, and a graduated cylinder, and a 50mL beaker-- were for measuring water volume (mL).   The tools used to determine the precision and accuracy were an electric scale, the provided 5 pieces of glassware, an extra beaker, a calculator, and 10 mL of H2O or water (distilled) per trial. The way to test the accuracy of a tool was to find how close the experimental volume of water in the given glassware was to the given theoretical volume, 10mL. Volume can be calculated with the formula mass/density = volume with the knowledge that water has a theoretical density of 0.997 g/mL under the lab conditions provided. To find

I looked over the instructions one last time and decided not to bother with them. It’s not like I couldn’t understand them – they were for a simple 8th grade science experiment, and I was an 8th grader with an interest in science. My problem with them was that they called for me to waste an entire hour moving a single thermometer between several different flasks of water. The different colored flasks were to be heated by an incandescent lightbulb, and the data I was supposed to gather by hand would reveal the exact nature of the relationship between the color of each flask and the amount of energy it absorbed. The concept of the experiment intrigued me, but I just couldn't accept the fact that I would have to manually track the temperature of each flask.

A circle of cardboard big enough to fit snugly just under the rim of a cup was cut out and placed slightly below the rim of one cup. The cup with the cardboard lid was stacked inside the other cup. A hole in which the thermometer could fit snugly was poked into the cardboard lid, and aluminum foil with a hole of the same size was placed over the cups to provide extra insulation. The commercial calorimeter provided for the experiment and two thermometers were also