Se recopilaron los datos siguientes de la velocidad de...

Se recopilaron los datos siguientes de la velocidad de desaparición de $\mathrm{NO}$ en la reacción $2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \longrightarrow 2 \mathrm{NO}_2(\mathrm{~g})$ : $$ \begin{array}{llll} \hline \text { Experimento } & {[\mathrm{NO}](M)} & {\left[\mathrm{O}_2\right](M)} & \text { Velocidad inicial }(\mathrm{M} / \mathrm{s}) \\ \hline 1 & 0.0126 & 0.0125 & 1.41 \times 10^{-2} \\ 2 & 0.0252 & 0.0250 & 1.13 \times 10^{-1} \\ 3 & 0.0252 & 0.0125 & 5.64 \times 10^{-2} \\ \hline \end{array} $$ (a) ¿Cuál es la ecuación de velocidad de la reacción? (b) ¿Cuáles son las unidades de la constante de velocidad? (c) ¿Cuál es el valor promedio de la constante de velocidad calculado con base en los tres conjuntos de datos?

Se recopilaron los datos siguientes de la velocidad de desaparición de $\mathrm{NO}$ en la reacción $2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \longrightarrow 2 \mathrm{NO}_2(\mathrm{~g})$ :
$$
\begin{array}{llll}
\hline \text { Experimento } & {[\mathrm{NO}](M)} & {\left[\mathrm{O}_2\right](M)} & \text { Velocidad inicial }(\mathrm{M} / \mathrm{s}) \\
\hline 1 & 0.0126 & 0.0125 & 1.41 \times 10^{-2} \\
2 & 0.0252 & 0.0250 & 1.13 \times 10^{-1} \\
3 & 0.0252 & 0.0125 & 5.64 \times 10^{-2} \\
\hline
\end{array}
$$
(a) ¿Cuál es la ecuación de velocidad de la reacción?
(b) ¿Cuáles son las unidades de la constante de velocidad? (c) ¿Cuál es el valor promedio de la constante de velocidad calculado con base en los tres conjuntos de datos?

Key Concepts

Rate Law

The rate law is an equation that relates the reaction rate to the concentrations of the reactants, where each concentration is raised to a power that represents its order in the reaction. It typically takes the form rate = k [A]^m [B]^n, and the exponents m and n indicate how sensitively the rate responds to changes in the reactants' concentrations.

Experimental Determination of Reaction Orders

Reaction orders are not always the same as the stoichiometric coefficients in a balanced equation; they must be determined experimentally. The method of initial rates is one common technique, where experiments measure how changes in individual reactant concentrations affect the initial rate, allowing one to deduce the order with respect to each reactant.

Average Rate Constant Calculation

When multiple experiments are conducted to determine the rate constant, each experiment provides an individual value of k. Averaging these values is a method to minimize experimental error, giving a more reliable overall estimate for k. This involves calculating k from each set of data using the rate law, and then computing the mean of these values.

Units of the Rate Constant

The units of the rate constant (k) depend on the overall order of the reaction. In the rate law equation, k must have units that, when multiplied by the concentration terms raised to their respective orders, yield the units of the rate (typically molarity per second). For instance, for an overall reaction order of n, the units of k will be M^(1-n) s^(?1).

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