Endothtermic And Exothermic Reaction Lab Report

Reaction 3- 1. Obtained a clean and dry test tube and placed a small amount ( about the size of a jelly bean) of ammonium carbonate into the test tube.

The main objective of this experiment is to differentiate between a physical change and a chemical change.

In this experiment, the ratio of anhydrous sodium carbonate to water is An endothermic reaction is characterised by the absorption of energy from the surroundings. This typically involves heat energy, which causes a decrease in temperature in the reaction and the surroundings. Examples of

A chemical reaction is when substances (reactants) change into other substances (products). The five general types of chemical reactions are synthesis (also known as direct combination), decomposition, single replacement (also known as single displacement), double replacement (also known as double displacement), and combustion. In this lab, the five general types of chemical reactions were conducted and observations were taken before, during, and after the reaction. Then the reactants and observations were used to determine the products to form a balanced chemical equation. The purpose of this lab was to learn and answer the question: How can observations be used to determine the identity of substances produced in a chemical reaction?

Endothermic reactions are accompanied by the absorption of heat. The dissolving of ammonium nitrate in water is an example of an endothermic reaction. The solution resulting from this mixture is colder than either the ammonium nitrate or the water. This is the simple explanation of what happens in an instant ice pack. The more detailed information will be discussed in the following paragraphs.

It was known that a reaction had occurred as there was the formation of new substances from the existing elements such as hydrogen. This was an exothermic reaction as it produced heat which was another factor contributing to the increased reaction rate.

This reaction is exothermic, meaning it releases heat when reactants are converted into products. The negative change in enthalpy (∆H° = -36,757 J) for this reaction indicates that the reaction is losing heat to its surroundings.

Purpose: The purpose of this experiment is to observe a variety of chemical reactions and to identify patterns in the conversion of reactants into products.

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.

As a result, this reaction is spontaneous at all temperatures. (8 points) Score 2. Consider the following reaction occurring in a closed chemical system. Assume that this reaction is at equilibrium and that in general the reaction to the right is favored.

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

The literature value for the enthalpy change of the last reaction which was provided by our teacher is -97 kJ mol-1. Agreeing this value, our result can be considered accurate.

The main objective of this experiment was to calculate the enthalpy of the reaction for the decomposition of hydrogen peroxide as well as measure the heat capacity in regard to the neutralization of a strong base and strong acid. Additionally, data was graphed in order to find the change in time relating to temperature vs. time. A calorimeter was made so that the temperatures of these reactions could be monitored and recorded, as well as allow us to complete calculations. Overall the results proved to be decent as there was a percent error for enthalpy of only 7.63%, and it was found that our calculations were accurate.

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.

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.