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Chapter 14: Problem 11

What two factors determine whether a collision between two reactant molecules will result in reaction?

Short Answer

Expert verified
The two factors are sufficient energy and proper orientation.

Step by step solution

01

Understanding Collision Theory

Collision theory states that for a chemical reaction to occur, reactant molecules must collide with each other.
02

Identifying Key Factors

There are two key factors that determine whether a collision between reactant molecules will lead to a reaction: sufficient energy and proper orientation.
03

Exploring Sufficient Energy

The molecules must collide with enough energy to overcome the activation energy barrier of the reaction. This is known as the energy threshold needed for the reaction to proceed.
04

Exploring Proper Orientation

Alongside sufficient energy, the molecules must collide with the correct orientation, so that reactive parts of the molecules interact effectively to form products.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Activation Energy
In the world of chemistry, activation energy is the minimum amount of energy that reactant molecules need to successfully collide and trigger a chemical reaction. Think of it as a barrier that must be overcome for a reaction to occur.
Imagine rolling a ball up a hill. The top of the hill represents the activation energy. Only when the energy is enough to get the ball over the hill, will it roll down the other side, much like a reaction proceeding. If the molecules in a collision do not have enough energy to surpass this barrier, the reaction will simply not happen.
Some important points about activation energy include:
  • Reactions with high activation energies require more energy input to occur.
  • Lowering the activation energy (such as with a catalyst) can increase the rate of reaction, as more molecules will have sufficient energy to react.
Chemical Reaction
A chemical reaction is a process where reactant molecules collide and transform into product molecules. This transformation involves breaking chemical bonds in the reactants and forming new ones to create products.
Reactions are meticulous processes, and they rely a lot on both energy and structural alignment. Merely colliding is not enough. Reactants must strongly interact; thus, they need to possess the needed energy and correct molecular structure during collision.
Here鈥檚 what influences chemical reactions:
  • Collision Frequency: More collisions can increase the reaction rate but without guaranteeing reaction.
  • Reactant Concentration: More reactant molecules can lead to higher chances of collisions.
  • Temperature: Higher temperatures increase the kinetic energy of the molecules, raising both the collision frequency and energy.
Molecular Orientation
Molecular orientation plays a crucial role in determining whether a collision will result in a chemical reaction. Even with sufficient energy, if molecules do not collide in the right orientation, the reaction might not occur.
Imagine two puzzle pieces that need to fit together perfectly. If they approach each other from the wrong angle, they won鈥檛 interlock. Similarly, for molecules, certain atoms or parts need to meet correctly to form bonds necessary for product formation.
Key points about molecular orientation include:
  • Effective orientation allows the reaction to proceed by aligning reactive sites.
  • Steric factors: Bulky groups around the reactive sites can prevent proper orientation.
  • Slight changes in molecular structure might dramatically affect orientation and reaction efficiency.

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Most popular questions from this chapter

List the four variables or factors that can affect the rate of reaction.

The chemical reaction \(\mathrm{A} \longrightarrow \mathrm{B}+\mathrm{C}\) has a rate constant that obeys the Arrhenius equation. Predict what happens to both the rate constant \(k\) and the rate of the reaction if the following were to occur. a. a decrease in temperature b. an increase in the activation energy of the forward and reverse reactions c. an increase in both activation energy and temperature

Azomethane, \(\mathrm{CH}_{3} \mathrm{NNCH}_{3}\), decomposes according to the following equation: $$ \mathrm{CH}_{3} \mathrm{NNCH}_{3}(g) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{6}(g)+\mathrm{N}_{2}(g) $$ The initial concentration of azomethane was \(1.50 \times 10^{-2}\) mol/L. After \(7.00\) min, this concentration decreased to \(1.01 \times\) \(10^{-2} \mathrm{~mol} / \mathrm{L}\). Obtain the average rate of reaction during this time interval. Express the answer in units of \(\mathrm{mol} /(\mathrm{L} \cdot \mathrm{s})\).

Compare the half-life equations for a first-order and second-order reaction. For which reaction order is the value of the half-life independent of the reactant concentration?

The reaction $$ \mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \longrightarrow 2 \mathrm{HI}(g) $$ may occur by the following mechanism: $$ \mathrm{I}_{2} \underset{k_{-1}}{\stackrel{k_{1}}{ }} 2 \mathrm{I} $$ (fast, equilibrium) $$ \mathrm{I}+\mathrm{I}+\mathrm{H}_{2} \stackrel{k_{2}}{\longrightarrow} 2 \mathrm{HI} $$ What rate law is predicted by the mechanism?
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