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Answer :
Final answer:
In order to accurately answer the student's question, more detailed information on the type of reaction order and the rate constant are needed. From the context, we do understand that the concentration of PCA, a reactant, should decrease over time. However, we need a little more information on the reaction specifics to give a numerical answer.
Explanation:
The subject of the question is related to the concept of chemical kinetics, with a focus on the subject of concentration of reactants over time and the effect of temperature on reaction rates. It is noted from the provided data that the concentration of PCA increases with higher temperatures. However, to determine the concentration of PCA at 40 hours at 97.3 °C, we would need data about the rate of reactions.
Under normal circumstances, you can calculate the concentration change over time by using a rate law, which usually has the form Rate = k [A]^m [B]^n, where [A] and [B] are the concentrations of the reactants and m and n are their respective reaction orders. Given that we are discussing concentration at a specific time, we're discussing zeroth, first, or second-order reactions, each with specific mathematical expressions and units for rate constant (k). However, the question doesn't give sufficent information to determine the reaction order or the rate constant, which are needed for the exact calculation.
Overall though, we know that if the starting concentration of PCA is 1.5M at 97°C, the concentration should be decreasing over time, given that PCA is a reactant and is being consumed in the process of the reaction.
Learn more about Chemical Kinetics here:
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