A Report On Chemical Equilibrium

The reaction "ICE" table demonstrates the method used in order to find the equilibrium concentrations of each species. The values that come directly from the experimental procedure are found in the shaded regions. From these values, the remainder of the table can be completed.

Changes in the rate of reaction can be described in terms of chemical equilibrium. “Chemical equilibrium is a state in which the forward and reverse reactions take place at the same rate” (Wilbraham et al, 2002). 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 is a simple equation that doesn’t properly prove the reaction. It is very complex and starts with this:

A chemical reaction is a process that involves change of the molecular or ionic structure of a substance, as opposed to a change in physical form or a nuclear reaction. The key concepts of a chemical reaction are:

1) Since the [OH⁻] would double, half the required number of drops would be needed.

This shows Le Chatelier’s principle as the system was able to neutralize the disturbance from its equilibrium.In this case, the change was the addition of molecules to the reactants. This caused an increase in the number effective collisions between the reactant’s molecules. Also, this raised the rate of the forward reaction. The system then has an increased amount of reactants and therefore has to travel in the forward direction to make extra products. This occurred in order to return the system to equilibrium by removing some of the excess reactants. By shifting in the forward direction, more products are being produced by the excess reactants. This ensures that the forward and reverse reaction rates are equal, which brings the system back to a state of

Molecules are still in motion, but there is no net change when dynamic equilibrium is reached.

In this experiment it was observed that not all chemical reactions occur at the same rate. Chemical reactions occur when one or more substances are changed into other substances. The properties of a chemical reaction require three things. First, they need a source of energy for molecules to encounter each other. Second, they require to proceed at a steady rate. Third, they must proceed in a particular direction until they reach equilibrium. There are two types of chemical reactions that can occur: endergonic and exergonic reactions. In these reactions there are both reactants and products. In exergonic reactions the reactants (starting materials of a reaction) are higher than the products (results of a reaction). This is opposite for endergonic

To learn about balancing chemical equations and law of conservation of mass in chemical reactions

This is my assignment one for the course CHE 432 at Arizona State University. The instructor for this class Dr. Burrows. Assignment one is due on Wednesday, August 30, 2017. There is no progress for date as this is the first assignment for the course. The assignments in this course will help me learn about chemical processes.

Dynamic Equilibrium: Two offsetting processes occur at equal rates, producing a state of balance where no net changes is observed.

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