Mechanical Work of Heat Lab Report Essay

The dependent variable in the experiment was the temperature and energy absorbed by the water.

Purpose: To become familiar with the International System of Units and common laboratory equipment and techniques. To learn how to determine volume, mass, length, and temperature of a wide variety of items. To learn how to calculate density and concentration of dilutions.

Twenty minutes and the temperature was at 30 ° C. After twenty-five minutes it was at 29 ° C. Thirty minutes and the temperature was still at 29 ° C. The experimenter noticed with the lamp on for thirty minutes the temperature overall increased 17°. With the lamp off for thirty minutes the temperature overall decreased 7°. The experimenter realized that it this proves sand heats up at a more rapid pace than water. After all the temperatures were recorded the experimenter unplugged the lamp. Removed thermometers from all the cans, carefully wiped and placed each can in the appropriate tray. The experimenter then emptied the sand into the bag of sand, and emptied the water into the sink and put the can in the tray marked empty water cans. Finally the experimenter took the lamp back to where it was found.

You have the mass of water from calculation #9, the specific heat of water is 4.184 J/g(oC), and the temperature change of water

A. Water boils at 100°C at sea level. If the water in this experiment did not boil at 100°C, what could be the reason?

Abstract: This experiment introduced the student to lab techniques and measurements. It started with measuring length. An example of this would be the length of a nickel, which is 2cm. The next part of the experiment was measuring temperature. I found that water boils around 95ºC at 6600ft. Ice also has a significant effect on the temperature of water from the tap. Ice dropped the temperature about 15ºC. Volumetric measurements were the basis of the 3rd part of the experiment. It was displayed during this experiment that a pipet holds about 4mL and that there are approximately 27 drops/mL from a short stem pipet. Part 4 introduced the student to measuring

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Purpose: To utilize a calorimeter correctly to find the enthalpy changes in two different reactions. The purpose was also to use concepts of specific heat to observe the relationship between temperature observations and heat transfer. Then, use the equations to see the relationship between change in energy and the amount of substance involved. Use Hess’ law to determine the change in energy.

Part 1: After reading the various information given, I gathered different objects and measured them using both centimeters and millimeters then converted them to meters. Next, I recorded the temperature of hot tap water and boiling water as

From the Melting point experiment, it was set to classify which substance has High melting point and which has low melting point. According to the results above we identified that Compound A has a high melting point and compound B has a low melting point. According to the Pre lab, Compound B was identified as Glucose (C6H12O6) and Compound A was identified as Sodium Chloride (NaCl). With the Conductivity experiment, the first part was to find out the conductivity in Solution state, Substance A conducted electricity and also changed the color of the solution and Substance B did not have any conductivity. With the second part of Conductivity test, tried to check the conductivity in molten state. The Bunsen burner was used to melt the compounds

In part A of the experiment we added 100 degree Celsius water to room temperature and tracked the temperature of the mixture to see how much it changed. Using this information we were able to calculate how much energy was given off by the how water and how much energy was absorbed by the cold water. The difference of the absolute values of these two values divided by the difference in temperature gave us the calorimeter constant. The calorimeter constant is an important value because it allow us to calculate how much energy is absorbed by the calorimeter in other reactions. Our calorimeter constant makes sense because it is a smaller value and with the colorimeter being Styrofoam, and insulator, the amount of heat absorbed by the calorimeter

We will be using 6 different fuels to heat up 100ml of water, and find out the changes of the temperature. We will measure the temperatures of the water before and after the experiment. We will burn heat the water for exactly 2 minutes, and check the changes in temperature. The change in temperature will allow us to work out the energy given off the fuel by using this formula:

Introduction: The theory behind this experiment is the heat of a reaction (∆E) plus the work (W) done by a reaction is equal to

Heat is a form of energy that is transferred between two substances at different temperatures. The flow of the energy is from the object of higher temperature to the object of lower temperature. The heat is measured in units of energy, usually calories or joules. Temperature on the other hand, is how cold or hot an object is. The temperature is the average kinetic energy per molecule of a substance. This is measured in degrees on the Celsius or Fahrenheit or in Kelvins.

Introduction: Every chemical change is accompanied by a change in energy usually in the form of heat. If heat is evolved, the reaction is exothermic, and if heat is absorbed, the reaction is endothermic. The energy change of a reaction that occurs at constant pressure is called the heat of reaction or the enthalpy of reaction (ΔHr). This quantity of heat is measured experimentally by allowing the reaction to occur in a calorimeter. In this experiment you will determine the heat of neutralization when an acid and a base react to form 1 mole of water. In a perfect calorimeter, heat is exchanged only between the reaction and the calorimeters water. Technically, some heat may may be absorbed the calorimeter. All calorimeters exchange some heat with its environment. This amount of heat is called the calorimeters heat capacity (the amount of of heat required to raise its temperature 1∘Celsius). We are going to “pretend” that our calorimeter is the perfect calorimeter.