Lab Report On Calorimeter Lab

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

In order to measure the heats of reactions, add the reactants into the calorimeter and measure the difference between the initial and final temperature. The temperature difference helps us calculate the heat released or absorbed by the reaction. The equation for calorimetry is q=mc(ΔT). ΔT is the temperature change, m is the mass, c is the specific heat capacity of the solution, and q is the heat transfer. Given that the experiment is operated under constant pressure in the lab, the temperature change is due to the enthalpy of the reaction, therefore the heat of the reaction can be calculated.

For q, you found how much heat was gained by the water so you know that same amount of heat was lost by the metal. Therefore, qmetal = -qwater. The mass of the sample was recorded from the baggie. The temperature change

The control experiment for this investigation will be the experimental setup of 5 trials using 5oC as the temperature. All the steps in the method will be followed.

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

Use your results in Data Tables 1 and 2 and the information provided in the Background section to calculate the amount of heat produced per gram (in Calories/gram) for each food and record this value for each food type.

The room temperature was measured throughout the lab and kept constant at 24°C (+/- 1°C), as the lab was conducted during the same time of

1. A constant volume must be kept in order to maintain reliable data and keep it directly proportional to the number of reactants consumed. Also, the results table can easily compare the changes in temperature and not be skewed. If you add a couple more milliliters to the experiment, it could produce a higher or lower temperature.

A metal sample weighing 45.2 g and at temperature of 100.0 ˚C was placed in a calorimeter containing

To improve the experiment, the methodology could be improved by having an efficient calorimeter to retain as much heat as possible, rather than just a tin can. Additionally, more trials for each of the experiments could be conducted to ensure correct and precise data is collected to determine more accurate conclusions.

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.

The styrofoam cups were used to store the acid (cup was labeled A) and base (cup was labeled B) prepare for them to be mixed. A lid was put on cup A and then the temperature probe was inserted to begin to measure the temperature

Background: Energy changes occur in all chemical reactions; energy is either absorbed or released. If energy is released in the form of heat, the reaction is called exothermic.

To achieve this, the final value from each thermocouple was set to be equal to the warm water bath temperature (370C), and the initial reading was set equal to the ice water bath temperature. Thus, for each thermocouple an equation was obtained using the two points to convert voltage readings to temperature. An example of the calibration for one of the thermocouples is shown in Appendix II.

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.