Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please see the attached equation and pictures for question
![### Chemical Equilibrium and Rate of Reaction
**Chemical Equation:**
\[ \text{N}_2(\text{g}) + 3 \text{H}_2(\text{g}) \rightarrow 2 \text{NH}_3(\text{g}) \]
This is the balanced equation for the synthesis of ammonia (NH₃) from nitrogen (N₂) and hydrogen (H₂) gases.
**Rate Expression:**
\[ \text{(rate expression)} \quad \text{Rate} = \]
The rate expression is a mathematical equation that describes the rate of a reaction in terms of the concentration of its reactants. For the synthesis of ammonia, the rate would typically be given as:
\[ \text{Rate} = k [\text{N}_2]^m [\text{H}_2]^n \]
Where:
- \(k\) is the rate constant.
- \([\text{N}_2]\) and \([\text{H}_2]\) are the concentrations of nitrogen and hydrogen, respectively.
- \(m\) and \(n\) are the orders of reaction with respect to each reactant, which are determined experimentally.
This rate law implies that the reaction rate is dependent on the concentrations of N₂ and H₂. However, the exact form of the rate law is determined experimentally.
### Understanding the Reaction:
- This reaction is an example of a combination reaction where two or more reactants combine to form a single product.
- On the molecular level, one mole of nitrogen reacts with three moles of hydrogen to produce two moles of ammonia.
- This process is critical in the industrial production of ammonia, known as the Haber process, which is fundamental for producing fertilizers.
### Graphs/Diagrams:
- There are no graphs or diagrams in the provided image. If there were, they would typically illustrate the concentration changes of the reactants and products over time, the activation energy of the reaction, or other kinetic parameters.
Stay tuned for further details and explanations on rate expressions and how they are experimentally determined.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4f7442e5-ed1a-4154-ba5d-4813abad6cff%2Fab1507ed-b6c0-4b0d-8348-9259e15d65dc%2F5u42ii8.png&w=3840&q=75)
Transcribed Image Text:### Chemical Equilibrium and Rate of Reaction
**Chemical Equation:**
\[ \text{N}_2(\text{g}) + 3 \text{H}_2(\text{g}) \rightarrow 2 \text{NH}_3(\text{g}) \]
This is the balanced equation for the synthesis of ammonia (NH₃) from nitrogen (N₂) and hydrogen (H₂) gases.
**Rate Expression:**
\[ \text{(rate expression)} \quad \text{Rate} = \]
The rate expression is a mathematical equation that describes the rate of a reaction in terms of the concentration of its reactants. For the synthesis of ammonia, the rate would typically be given as:
\[ \text{Rate} = k [\text{N}_2]^m [\text{H}_2]^n \]
Where:
- \(k\) is the rate constant.
- \([\text{N}_2]\) and \([\text{H}_2]\) are the concentrations of nitrogen and hydrogen, respectively.
- \(m\) and \(n\) are the orders of reaction with respect to each reactant, which are determined experimentally.
This rate law implies that the reaction rate is dependent on the concentrations of N₂ and H₂. However, the exact form of the rate law is determined experimentally.
### Understanding the Reaction:
- This reaction is an example of a combination reaction where two or more reactants combine to form a single product.
- On the molecular level, one mole of nitrogen reacts with three moles of hydrogen to produce two moles of ammonia.
- This process is critical in the industrial production of ammonia, known as the Haber process, which is fundamental for producing fertilizers.
### Graphs/Diagrams:
- There are no graphs or diagrams in the provided image. If there were, they would typically illustrate the concentration changes of the reactants and products over time, the activation energy of the reaction, or other kinetic parameters.
Stay tuned for further details and explanations on rate expressions and how they are experimentally determined.
![**Rate of Change of Nitrogen Concentration**
---
**What is the rate of change of \([N_2]\) per time? \(\Delta [N_2] / \Delta t =\)**
---
In this transcription, we are exploring the concept of the rate of change of nitrogen concentration, denoted as \([N_2]\), with respect to time. Understanding this rate is crucial in various fields such as chemistry and environmental science, where nitrogen plays a significant role in reactions and ecosystem dynamics.
The notation \(\Delta [N_2] / \Delta t\) represents the change in nitrogen concentration (\(\Delta [N_2]\) in moles per liter) over the change in time (\(\Delta t\)). This ratio provides scientists and students with insight into how quickly or slowly the nitrogen concentration is varying within a given time period.
This concept can be applied in practical scenarios such as predicting reaction rates in chemical processes, understanding ecological balances, or even monitoring atmospheric nitrogen levels.
Exploring further into this topic would involve discussing the methods to measure \([N_2]\), experimental setups, and the importance of accurate time interval recording.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4f7442e5-ed1a-4154-ba5d-4813abad6cff%2Fab1507ed-b6c0-4b0d-8348-9259e15d65dc%2Fdv9ie49.png&w=3840&q=75)
Transcribed Image Text:**Rate of Change of Nitrogen Concentration**
---
**What is the rate of change of \([N_2]\) per time? \(\Delta [N_2] / \Delta t =\)**
---
In this transcription, we are exploring the concept of the rate of change of nitrogen concentration, denoted as \([N_2]\), with respect to time. Understanding this rate is crucial in various fields such as chemistry and environmental science, where nitrogen plays a significant role in reactions and ecosystem dynamics.
The notation \(\Delta [N_2] / \Delta t\) represents the change in nitrogen concentration (\(\Delta [N_2]\) in moles per liter) over the change in time (\(\Delta t\)). This ratio provides scientists and students with insight into how quickly or slowly the nitrogen concentration is varying within a given time period.
This concept can be applied in practical scenarios such as predicting reaction rates in chemical processes, understanding ecological balances, or even monitoring atmospheric nitrogen levels.
Exploring further into this topic would involve discussing the methods to measure \([N_2]\), experimental setups, and the importance of accurate time interval recording.
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