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Chapter 2: Problem 34

In order for the hydrogen and nitrogen to react, there must be A. effective collisions between the hydrogen and nitrogen gases so as to cause a rearrangement of atoms B. a sufficient amount of ammonia present to form the hydrogen and nitrogen C. contact between the hydrogen and nitrogen atoms D. smaller amounts of hydrogen and nitrogen present

Short Answer

Expert verified
Option A: Effective collisions are needed for hydrogen and nitrogen to react.

Step by step solution

01

- Understand the Question

Identify what the question is asking. Here, the question pertains to the conditions required for hydrogen and nitrogen to react effectively.
02

- Recall Reaction Conditions

Recall that for a chemical reaction to occur, there must be effective collisions between reactant molecules that have enough energy to break existing bonds and form new ones.
03

- Analyze Each Option

Consider each option given:A. Effective collisions - This is often necessary for reactions as it involves proper energy and orientation.B. Ammonia presence - This is not a prerequisite for the reaction.C. Contact between atoms - Contact alone is not enough without effective collisions.D. Smaller amounts - This is not typically required for reactions to occur.
04

- Eliminate Incorrect Options

Eliminate options B, C, and D as they do not align with the necessary conditions for effective chemical reactions.
05

- Choose the Correct Answer

Based on the analysis, the correct answer is option A, which states that effective collisions are required for causing rearrangement of atoms.

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Key Concepts

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

Effective Collisions
For a chemical reaction to occur, molecules must collide in a manner that leads to the rearrangement of their atoms. These specific kinds of collisions are what we refer to as effective collisions. Effective collisions are not just random; they must occur with the correct orientation and sufficient energy for the reactants to form new products. Without effective collisions, the reactant molecules may simply bounce off each other without any reaction taking place. In other words, just having molecules bump into each other isn’t enough; they must collide the right way.
Energy Requirements
Another crucial aspect to understand is the energy needed for these reactions to happen. In chemical reactions, bonds between atoms in the reactant molecules must be broken, and new bonds must be formed to create the products. This requires a certain amount of energy, typically referred to as activation energy, which the molecules must possess during their collisions.
This means that even if collisions occur with the correct orientation, they still need to have enough energy to overcome the activation energy barrier. Without this energy, the effective collisions won't result in a chemical reaction.
Reactant Molecules
Reactant molecules are the starting substances in a chemical reaction. In the context of our exercise, the reactant molecules are hydrogen and nitrogen. For these molecules to react and form ammonia, several conditions have to be met:
  • The molecules must collide effectively.
  • They must possess enough energy to overcome the activation energy.
  • They must maintain the proper orientation during collisions.

If these conditions are satisfied, the reactant molecules will interact to form new chemical bonds, leading to the formation of new products, in this case, ammonia. Understanding the role and behavior of reactant molecules is essential for predicting and controlling chemical reactions.

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