The Effect Of Chemical Reactions On Temperature, Enthalpy, And Specific Heat

Abstract: An ice calorimeter was used to study the reaction of magnesium metal and 1.00M

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.

Examine a piece of nichrome wire. On the data sheet, record the color and the luster of the metal. Use a forceps to hold the wire in the flame of your burner for about two minutes (recall where the hottest part of the flame is located). Describe the appearance of the wire while held in the hottest part of the flame. Allow the wire to cool and reexamine it. From your observations, determine if there was a physical or a chemical change. Give specific reasons for your conclusions. Save the nichrome wire for step #2.

We were also able to conclude that when you combine equal parts of an acid and base you can expect to see a higher temperature change than you would if you added more parts of a base than a acid. Our reasoning behind this conclusion is that when we added 10 mL of both solutions that temperature increased by 5ºc, but when we added 15 mL of NaOH and only 5 mL of CH3COOH there was only a temperature increase of 3ºc. In correlation, we calculated that when you have equal parts of acid and base, the ΔHrxn will be higher than when you use more parts base than

A chemical change is a change that alters the identity of a substance. A chemical change can be identified by five things: change in mass, formation of a precipitate, release of heat and/or light, color change, or giving off gas.

In this unit we have conducted research and experiments on our chosen reactions to create the highest exothermic reaction for the The Heat-and-Eat meal pack will use a chemical reaction that involves two reactants. Reactant 1 is a solid and Reactant 2 is a liquid.

If 10.0g of solid baking soda is poured into 30 mL of citric acid, then a reaction will occur and an increase in temperature will be observed. Whereas, if a piece of magnesium metal is added to 30 mL of Hydrochloric Acid, then a reaction will occur and an increase in temperature will be observable. For Part 3 of the experiment, if 50 mL of tap water is placed in a can 2.5 cm inches above a burning marshmallow, then through the process of calorimetry the energy content of the marshmallow should be 5.0kJ/g (the value provided by the United States Department of Agriculture).

Chemical reactions that absorb energy are called endothermic reactions, these reactions are observed by a decrease in temperature of the reaction mixture.

This paper is about chemical reactions and chemical reaction types. All the data gathered was from conducting multiple experiments. Each experiment was performed carefully and analyzed to obtain the necessary information for the paper. That information included the four signs of a chemical change, the rnx type, and more.

However, the calculated value of specific heat, i.e. 12.91 j/g0C, was relatively larger than expected due to some possible sources of errors. One of the possible sources of error in the experiment was possible loss of heat through the hole where the thermometer was initially inserted. In addition, heat loss may have occurred when the metal was transferred from the heated beaker to the calorimeter. To reduce these errors, the experiment should be conducted in a more controlled

Conclusion As concluded at the end of the experiment,we have found that the combinations that not only had the greatest change in temperature, but also big observations were Hydrogen peroxide and and Dry yeast and Water and Ice. with changes of 15 and 31 degrees

This experiment was performed to determine the heat of neutralization between Hydrogen chloride (HCl) and Sodium hydroxide (NaOH). A temperature probe was used to measure the temperature of the reaction when the base (NaOH) was poured into the acid (HCl). The data was collected on logged on LoggerPro.

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

Purpose: To measure the heats of reaction for three related exothermic reactions and to verify Hess’s Law of Heat Summation.

Purpose: This lab taught procedures for determining heat of capacity of a calorimeter and measuring enthalpy of change for three reactions. It also enforced methods of analyzing data obtained through experimentation and calculating enthalpy. These procedures are used in the branch of thermodynamics known as thermochemistry which is the study of energy changes that accompany chemical reactions. Concepts from this lab can be used to determine the potential energy of a chemical reaction. Much of the energy people depend on comes from chemical reactions. For example, energy can be obtained by burning fuel, metabolizing of food or discharging a batter.