Chemical Kinetics Purpose The purpose of this experiment is to determine the rat

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Chemical Kinetics Purpose The purpose of this experiment is to determine the rate law and rate constant for the reaction of oxalic acid with permanganate Introduction Chemical Kinetics is a term used to describe the study of the rates of chemical reactions. Every chemical reaction takes time to occur, which can range from hours to femtoseconds. The rate of a chemical reaction can be determined by assessing the change in either reactant or product in a given time point. Regardless as to which compound is chosen to determine the rate, the answer will be the same; however, it is important to take into account the stoichiometric ratios of each component. For example, consider the following generic chemical reaction: aA bB cC dD The rate of reaction can be expressed as a function of each reactant and each product 1 ALA] 1 A[B] 1 AIC] 1 AID] Rate b At a At c At d At Note that for each reactant, the concentration is decreasing as the reaction occurs; therefore, to represent rate as a positive value, a negative sign in the rate definition is used. Conversely, the concentration of the products is increasing as the reaction proceeds; therefore, the change in concentration is positive. Measuring reaction rates can be done several ways, and involves being able to accurately measure the change in concentration of one of the reaction species over time. This experiment will utilize a visual change in color of one of the reactants used; however, since visual indications can be subjective (and therefore not entirely accurate), it is important to perform the experiment multiple times. In addition ce the color change would indicate that the concentration of the monitored reactant has reached zero, then this experiment will measure the average reaction rate for the experiment rate law for a chemical reaction describes how the rate of reaction relates to the concentration of r more of the reactants in a reaction. Using the same generic reaction as above, the rate law is written as follows Rate k[A] [B] In this equation, k represents a rate constant specific to the reaction, and x and y represent the reaction order for A and B, respectively. Note that X and y are NOT the stoichiometric coefficients for the reaction b. The values for the reaction order can ONLY be determined by experiment, not by the balanced cal equation

Explanation / Answer

1. Rate of reaction = -1/3 d[oxalic acid] /dt = -1/2 d [KMO4] / dt

2. Unit of rates of reaction moles L-1 second-1

3. Rate= K[oxalic acid] x [KMnO4]y

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