Answer:
En química, la reactividad de una especie química es su capacidad para reaccionar en presencia de otras sustancias químicas o reactivos (de diferente dominio químico).1
Se puede distinguir entre la reactividad termodinámica y la reactividad cinética. La primera distingue si la reacción está o no favorecida por entalpía (competencia entre energía y entropía), es decir si es una reacción espontánea o no. La segunda distingue si la reacción tendrá lugar o no en una escala de tiempo dada.
De esta forma, existen reacciones termodinámicamente favorables pero cinéticamente impedidas, como la combustión de grafito en presencia de aire. En casos así, la reacción se dará de una forma muy lenta o, directamente, no se producirá. Si una reacción se encuentra bloqueada cinéticamente, es posible lograr que se produzca alterando las condiciones de reacción o utilizando un catalizador.
La química orgánica y la química inorgánica estudian la reactividad de los distintos compuestos. La fisicoquímica trata de calcular o predecir la reactividad de los compuestos, y de racionalizar los mecanismos de reacción.
Explanation:
There are different kinds of angles. The measure of each exterior angle of the formation is 51.4.
<h3>What is a exterior angle in math?</h3>
The term exterior angle is known to be the angle that is found between a side of a polygon and that of an extended adjacent side.
The shape of the halftime is regular heptagon.
Note that a regular heptagon has 7 congruent sides and 7 congruent interior angles.
So the exterior angles are said to be congruent, based on the fact that angles supplementary to congruent angles are regarded as congruent.
So Let take n as the measure of each exterior angle.
7n = 360
n= 360/n
To Solve for n =51.4
Therefore, The measure of each exterior angle of the formation is 51.4.
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The rate of disappearance of O2(g) under the same conditions is 2.5 × 10⁻⁵ m s⁻¹.
<h3>What is the rate law of a chemical equation? </h3>
The rate law of a chemical reaction equation is usually dependent on the concentration of the reactant species in the equation.
The chemical reaction given is;
The rate law for this reaction can be expressed as:
![\mathbf{= -\dfrac{1}{2}\dfrac{d[NO]}{dt} = -\dfrac{1}{1}\dfrac{d[O_2]}{dt}= +\dfrac{1}{2}\dfrac{d[NO_2]}{dt}}](https://tex.z-dn.net/?f=%5Cmathbf%7B%3D%20-%5Cdfrac%7B1%7D%7B2%7D%5Cdfrac%7Bd%5BNO%5D%7D%7Bdt%7D%20%3D%20-%5Cdfrac%7B1%7D%7B1%7D%5Cdfrac%7Bd%5BO_2%5D%7D%7Bdt%7D%3D%20%2B%5Cdfrac%7B1%7D%7B2%7D%5Cdfrac%7Bd%5BNO_2%5D%7D%7Bdt%7D%7D)
Recall that:
- The rate of disappearance of NO(g) = 5.0× 10⁻⁵ m s⁻¹.
- Since both NO and O2 are the reacting species;
Then:
- The rate of disappearance of NO(g) is equal to the rate of disappearance of O2(g)
![\mathbf{= -\dfrac{1}{2}\dfrac{d[NO]}{dt} = -\dfrac{1}{1}\dfrac{d[O_2]}{dt}}](https://tex.z-dn.net/?f=%5Cmathbf%7B%3D%20-%5Cdfrac%7B1%7D%7B2%7D%5Cdfrac%7Bd%5BNO%5D%7D%7Bdt%7D%20%3D%20-%5Cdfrac%7B1%7D%7B1%7D%5Cdfrac%7Bd%5BO_2%5D%7D%7Bdt%7D%7D)
Thus;
The rate of disappearance of O2 = 2.5 × 10⁻⁵ m s⁻¹.
Therefore, we can conclude that two molecules of NO are consumed per one molecule of O2.
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