Reaction Order and Rate Laws

Topics: Rate equation, Chemical reaction, Reaction rate / Pages: 10 (2460 words) / Published: Mar 24th, 2014
Lab 3: Reaction Order and Rate Laws

Name: Student
Lab Partners: None
Date of Experiment: 16 March 2014
Location: My House
Course Number: CHE112

Abstract: When combining compounds, there are always two roles considered in the reaction. These are reactants and products. Reactants are the initial compounds before mixing. The products are synonymous with the term byproduct, or what remains when the reaction occurs. For example, Sodium (Na+) and Chlorine (Cl-) are mixed to create Sodium Chloride (NaCl) . In this example, sodium and chlorine are the reactants and sodium chloride is the product. The use of rate laws expresses the rate of a given reaction to produce a concentration of a reactant in a given chemical reaction such as described with sodium chloride. This is important because the use of rate laws can be used to calculate how much of a reactant is used and how quickly a reaction occurs based on the level of concentration of the reactants. Knowing this, chemists can speed up or slow down reactions which is useful if the initial reaction time is extremely long or requires an exorbitant about of products to produce the desired results in the reaction. Certain factors can actually speed up the reaction rate. The factors include temperature, pressure, concentrations of the reactants, the nature of the reaction (polar vs non-polar) and the presence of a catalyst. The primary component outside of the reactant concentrations themselves is energy. Recalling the concept of Gibbs free energy as the total amount of energy used for the reactants to form products in redox chemistry one can summarize that energy can play as much of a role in chemical reactions as the concentrations of reactions. This is because reactions occur when the molecules of each product collide with one another. If there is enough energy, molecules of one reactant can be taken and/or gained by the other creating the products. This is why

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