Background A chemical equation that is in equilibrium will naturally balance itself out should either the products are the reactants be increased, or other stresses such as temperature and pressure are placed on it. However, as with a lever in physics, the fulcrum or balancing point is not always in the middle. In most cases, one side of the equation will be favored more. Ergo, the equation will try to balance to this point of equilibrium.
Materials
We did several different examples of chemical equilibriums using different stresses and conditions. This includes adding or removing reactants, changing temperature, or adding additional compounds. Our materials included a large variety of chemicals and equipment used to conduct our labs.
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The first lab was testing the equilibrium of hydrogen ions within brewed tea. We put tea in three different wells. One was left alone for a control, one had acetic acid added to it, and the other had sodium hydroxide added to it. The solution was stirred after each substance was added to the tea to ensure even distribution. After finishing and recording results and observations, the trays were rinsed and dried. The second lab was testing the equilibrium of starch, iodine, and starch-iodine complex. For this lab we needed heated water and cold water. We created a diluted starch mixture in two wells and placed water of different temperatures of each one. The change in temperature would cause stress in the equilibrium, meaning it would have to rebalance itself. The wells were again cleaned and dried to prepare for the next …show more content…
When in bonded, it turned a deep hue of purple. However, when they were separate the mixture was clear. We could see the change in this scenario when we changed the temperature by placing either heated water or iced water under the different wells. When the temperature was raised, the color was much lighter and more clear, implying that the starch and iodine were not forming the bonded complex. However, when the temperature was lowered, it because a very dark shade of purple, almost appearing to be black. In the equation we could see that the formation of the complex produced heat as well, which represents why it responds the way it does. If you treat heat as a product, then by raising the temperature it will try to balance itself by shifting the balance to the other side, forming separated iodine and starch. The opposite is also true, and this is because the reaction is exothermic in one direction, but can be treated as endothermic in the other
6-3: This process is used by cells to manufacture _biochemical energy from nutrients into adenosine triphosphate (ATP), and then release waste products__
In the study of chemical reactions, chemistry students first study reactions that go to completion. Inherent in these familiar problems—such as calculation of theoretical yield, limiting reactant, and percent yield—is the assumption that the reaction can consume all of one or more reactants to produce products. In fact, most reactions do not behave this way. Instead, reactions reach a state where, after mixing the reactants, a stable mixture of reactants
Procedure: In this experiment, various chemicals were mixed together, to determine a reaction. Using two drops from chemical 1 and two drops of chemical two, unless otherwise stated, then recording the type of physical reaction or color changes that occurred.
The main objective of this experiment is to differentiate between a physical change and a chemical change.
The materials used during the experiment included three plastic cups, three gummy bears, masking tape, marker, balance, calculator, tray, one plastic spoon, a measurement tray, and a ruler. The three plastic cups were used to hold the tap water, salt water, and sugar water. The masking tape and marker were used to label each cup with the
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?
Aim: The aim of the lab “Chemical Equilibrium” is to observe the effects of changes in concentrations of products and reactants on the position of the equilibrium of given chemical reactions.
During the experiment, two different techniques to disturb systems at chemical equilibrium are utilized. The first one is changing the concentration of one of more species that are involved
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.
Substances A and B have an appearance of a white solid like. Substances A and B were put into a test tube and on the Bunsen burner. As a result, B melted faster than A. A was slow to melt. The reason why B melted faster than A is because it has a lower boiling point than substance A which made it melt faster. It also shows that A needs more energy than B to be broken down.
36. Coefficients are written in front of the formulas of reactants and products to balance chemical
Objective(s): The reason for this experiment is to see how starch and iodine affect each other and how a plastic bag works similar to a membrane in certain situations.
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.
If the relative amount of reactants is altered, then the limiting reactant may change accordingly. For example, a balanced chemical equation of a certain reaction specifies that an equal number of moles of two substances A and B is required. If there are more moles of B than of A, then A is the limiting reactant because it is completely consumed when the reaction stops and there is an excess of B left over.
Chemical equilibrium is the study of change within a chemical reaction and how far it will go to reach a dynamic equilibrium (Burdge). Dynamic equilibrium is defined as the constant movement of species in a chemical reaction, gone to incompletion while the rates of production and consumption are equal (Kf = Kr ) (Burdge). It differs from static equilibrium in that species are constantly being consumed and produced, it is dynamic movement (Fox). The concentration of such species do not change, it remains constant (Fox). The rate at which species are being consumed and produced is known as the equilibrium constant (K) (Burdge). Due to the fact that the concentration