CHEMISTRY 1111 LAB MANUAL >C<
CHEMISTRY 1111 LAB MANUAL >C<
1st Edition
ISBN: 9781307092097
Author: Chang
Publisher: MCG/CREATE
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Chapter 10, Problem 10.50QP

The formation of H2 from two H atoms is an energetically favorable process. Yet statistically there is less than a 100 percent chance that any two H atoms will undergo the reaction. Apart from energy considerations, how would you account for this observation based on the electron spins in the two H atoms?

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Using the Arrhenius equation, it is possible to establish the relationship between the rate constant (k) of a chemical reaction and the temperature (T), in Kelvin (K), the universal gas constant (R), the pre-exponential factor (A) and the activation energy (Ea). This equation is widely applied in studies of chemical kinetics, and is also widely used to determine the activation energy of reactions. In this context, the following graph shows the variation of the rate constant with the inverse of the absolute temperature, for a given chemical reaction that obeys the Arrhenius equation. Based on the analysis of this graph and the concepts acquired about the kinetics of chemical reactions, analyze the following statements:              I. The activation energy (Ea) varies with the temperature of the system.   II. The activation energy (Ea) varies with the concentration of the reactants.        III. The rate constant (K) varies proportionally with temperature.    IV. The value of the…
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