Exothermic: Thermodynamics and Data Table

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

Step 3: Use the thermometer to identify and record the temperature for room temperature, in your refrigerator, in your freezer, and then research the temperature of boiling water (do not take this temperature) and record them in Table 2.

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

If the difference between the recorded times are more than 10%, add a third trial. Repeat these steps with each size beaker. Calculate the average time for each beaker and record the data. The next step of the lab exercise is determining the exact volume of the beakers used in the burn time experiment. Fill a beaker to the top with water. Carefully pour the water from the beaker into a graduated cylinder. Reading the meniscus, record the exact volume into a data sheet. Repeat this step with each size beaker until all volumes are recorded into the data sheet. The final process of the Graphing and Estimating lab is plotting the recorded data onto a graph. Using the data recorded for burn time, in seconds, place the data on the vertical axis. Use the horizontal axis for the volume in milliliters. With the data points plotted determine whether a straight line or a simple curve will best represent the data. Now, obtain a jar and determine the volume. Fill the jar to the top with water. Carefully pour the water into a graduated cylinder. Precisely record the data. Using the plotted data on the graph and the simple curve or straight line to predict how long it would take for the flame to burn out on the candle if it was covered with the jar that was just measured.

13. The temperature of the water was measured prior to the tube being placed in it and the temperature of the Hydrochloric Acid was measured after it 's temperature had adjusted.

13. Calculate the change in temperature for the water caused by the addition of the aluminum by subtracting the initial temperature of the water from the

This document is not meant to be a substitute for a formal laboratory report. The Lab Report Assistant is simply a summary of the experiment’s questions, diagrams if needed, and data tables that should be addressed in a formal lab report. The intent is to facilitate students’ writing of lab reports by providing this information in an editable file which can be sent to an instructor.

Use the same Elodea to conduct the other 4 trials for that same temperature, repeat steps 1-5 for each trial.

2. How did concentration and/or volume differences affect the heat change (q) for each trial?

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

In this experiment, we investigate the change in temperature caused by adding a chemical substance into the water and dissolving it. The results recorded in the table below show that our hypothesis is correct.

The lab used methods of calorimetry in order to measure the temperature change of reactions and calculate the changes in

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

3. Calculate the total heat released in each reaction, assuming that the specific heat of the solution is the same as for pure water (4.18J/gK). Use q=mcΔT. Show work here and record your answer in Data Table 2.