How Does Temperature Affect The Combustion Of A Copper Calorimeter

Before the experiment, several pieces of glass were put into an oven to dry, and the heat from the

    One possible source of error that can affect the results was that a mercury thermometer was used instead of an electronic one. The use of a mercury

In this science unit we had to keep 200 milliliters of boiling water hot as warm as possible for 20 minutes. For trial one we put tin foil all around flask so the heat waves would reflect back to the flask. Also we put tin foil on the top of the flask to stop convection because warm rises. So when the hot air rises we wanted the tin foil to reflect the hot air back into the flask. Then we were going to put the flask in in a wooden box with a small volume, but then keegan forgot to bring in the box so we had to put the flask with the tin foil around it in our ELA project.Then we put a ton of cotton balls all around the flask and tin foil to insulate the water in the flask. At the end of trial 1 we lost 15.7℃. One thing we did well is we kept the heat in by insulating with cotton balls. Another thing we did well was stopping convection by putting tin foil on the top.

In an article called “Heat Transfer by conduction” by Mike Brown, it states “Thermal energy in the vibrating particles or molecules is passed on to nearby particles in a process called conduction”. This explains to us the process of conduction in which it relates to our design because when we insert the thermometer into the warm water, our goal is to keep the water warm with our cup so that once the thermometer makes DIRECT contact with the warm water, it will heat up the thermometer and give us an exact temperature.

Both the can and the beaker, with an almond, the results are in between the values of 9-5. For example, the heat released by sample (cal) for the can was 9.054 cal and 5.628 cal; for the beaker it is 6.489 cal and 5.796 cal. Trial 2 is similar to each other compared to Trial 1; however, Trial 1 is higher than Trial 2. In addition, the beaker has the same experimental caloric content (calories per gram) for trial 1 and 2, but not for the can. For example, the experimental caloric content for the beaker are both 7 cal/g and for the can it is 9 cal/g and 6 cal/g. The nut substitute, goldfish crackers, has lower values compared to the almonds and cashews. For example, the experimental Cal/g for the goldfish crackers were both 0.001 Cal/g while for the almonds it is 0.009 Cal/g and 0.006 Cal/g and for the cashews it is 0.003 Cal/g and 0.005

releases the heat after the sun has set. One may think that this is a positive

The purpose of my experiment was to see how much energy was wasted in different types and wattages of lightbulbs through the output of heat. The initial objective of the project was to research the variety of lightbulbs available on the market today including their wattage and other important features pertaining to their operation before starting the experiment. The reports provided information that first helped me to formulate a plan to calculate heat energy, measured in calories. I was then able to subsequently convert the heat energy into joules which is a more commonly used unit of energy. This was accomplished by multiplying the amount of calories produced through

Further calibration of all the thermometers was also indicated within the article. Burns & Grove (2011) write that

b) An empty beaker was weighted. Then, water was filled in the beaker. The temperature was recorded at uniform intervals.

There is the term ‘surroundings’ which is used for the can itself holding the body of water, and for the room in which the practical experiment took place. It is known that any heat lost by the system must be absorbed by the surroundings, this is important for the surroundings referring to the room as it had much effect on the results. These effects are why the values in data and the consistency in the results have errors due to the calorimetry. The major calculations for calorimetry would be for the amount of heat absorbed by water. This is based off the calorimeter can’s surroundings of the water. The equation used

The purpose of the experiment is to determine the enthalpy of neutralization reactions by calorimetry. Calorimetry, is the science of measuring the amount of heat. All calorimetric techniques are therefore based on the measurement of heat that may be generated (exothermic process) or consumed (endothermic process). The device used for measuring the heat changes in this experiment is called calorimeter. A calorimeter is a Styrofoam cup is used as a calorimeter, because it is a container with good insulated walls to prevent heat exchange with the environment.

However, there is an outlier in the graph, so there was a systematic error for that value of ‘t’.

In this experiment, the data that has been collected using thermocouple that has been carried out in Mechanical Engineering Department pantry room, UPM shows into the graph. The graph of the data is shown as below.

There will be two main parts to this experiment. In the first part, we will study the power lost from a 0.35m brass cylindrical pin due to natural convection and radiation. This will be done by inspecting the input power and the temperature along different points on the pin. The different temperature points will give an idea on the loss of heat between specific sections. The second part will be concerned with studying the combine effect of natural convection/radiation and comparing it with the effects of forced convection/radiation. The latter can be observed by forcing air over the desired interface.

When the external temperature is higher than 40 °C, the difference between this temperature and the required degree inside (22 °C) is significant,