The central idea of the collision model is that molecules must collide in order to react. Give two reasons why not all collisions of reactant molecules result in product formation.

Short Answer

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The central idea of the collision model states that molecules need to collide in order to react. However, not all collisions result in product formation due to two main reasons: 1) insufficient energy, where colliding molecules don't possess enough activation energy to break the reactant bonds and form new ones in the products, and 2) incorrect orientation, where the reactant molecules' reactive sites don't interact with each other during the collision.

Step by step solution

01

Introduction to Collision Model

The collision model is a concept used to explain how chemical reactions occur between particles. According to this model, in order for a reaction to occur, the reactant molecules must collide with each other. However, not all collisions result in product formation. Now, let's discuss two reasons why not all collisions lead to a product.
02

Reason 1: Insufficient Energy

One main reason why not all the collisions result in product formation is the lack of sufficient energy. When reactant molecules collide, they need to possess enough energy (known as the activation energy) to break the chemical bonds in the reactants and form new bonds in the products. If the colliding molecules do not possess enough energy, the reaction does not occur, and there will be no product formation.
03

Reason 2: Incorrect Orientation

Another reason why not all collisions result in product formation is related to the orientation of the reactant molecules during the collision. For a reaction to occur, the reactant molecules must collide with a specific orientation, such that their reactive sites interact with each other. If the molecules collide with an incorrect orientation, the reaction won't take place and no products will be formed. In conclusion, the central idea of the collision model is that molecules need to collide in order to react. However, not all collisions form products because the reactant molecules might not have enough energy (activation energy) or the correct orientation during the collision.

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Most popular questions from this chapter

Upon dissolving \(\operatorname{InCl}(s)\) in \(\mathrm{HCl}, \mathrm{In}^{+}(a q)\) undergoes a disproportionation reaction according to the following unbalanced equation: $$ \mathrm{In}^{+}(a q) \longrightarrow \operatorname{In}(s)+\mathrm{In}^{3+}(a q) $$ This disproportionation follows first-order kinetics with a halflife of \(667 \mathrm{~s}\). What is the concentration of \(\mathrm{In}^{+}(a q)\) after \(1.25 \mathrm{~h}\) if the initial solution of \(\mathrm{In}^{+}(a q)\) was prepared by dissolving \(2.38 \mathrm{~g} \operatorname{InCl}(s)\) in \(5.00 \times 10^{2} \mathrm{~mL}\) dilute HCl? What mass of \(\operatorname{In}(s)\) is formed after \(1.25 \mathrm{~h}\) ?

Consider a reaction of the type \(\mathrm{aA} \longrightarrow\) products, in which the rate law is found to be rate \(=k[\mathrm{~A}]^{3}\) (termolecular reactions are improbable but possible). If the first half-life of the reaction is found to be \(40 . \mathrm{s}\), what is the time for the second half-life? Hint: Using your calculus knowledge, derive the integrated rate law from the differential rate law for a termolecular reaction: $$ \text { Rate }=\frac{-d[\mathrm{~A}]}{d t}=k[\mathrm{~A}]^{3} $$

Describe at least two experiments you could perform to determine a rate law.

Draw a rough sketch of the energy profile for each of the following cases: a. \(\Delta E=+10 \mathrm{~kJ} / \mathrm{mol}, E_{\mathrm{a}}=25 \mathrm{~kJ} / \mathrm{mol}\) b. \(\Delta E=-10 \mathrm{~kJ} / \mathrm{mol}, E_{\mathrm{a}}=50 \mathrm{~kJ} / \mathrm{mol}\) c. \(\Delta E=-50 \mathrm{~kJ} / \mathrm{mol}, E_{\mathrm{a}}=50 \mathrm{~kJ} / \mathrm{mol}\)

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