# Gas Phase Reaction MechanismOne possible mechanism for the gas phase reaction of hydrogen with nitrogen monoxide is:### Step 1: (Slow)\[ \text{H}_2(g) + 2 \text{NO}(g) \rightarrow \text{N}_2\text{O}(g) + \text{H}_2\text{O}(g) \]### Step 2: (Fast)\[ \text{N}_2\text{O}(g) + \text{H}_2(g) \rightarrow \text{N}_2(g) + \text{H}_2\text{O}(g) \]## Questions1. **What is the equation for the overall reaction?** Use the smallest integer coefficients possible. If a box is not needed, leave it blank. \[ \text{[Box]} + \text{[Box]} \rightarrow \text{[Box]} + \text{[Box]} \]2. **Which species acts as a catalyst?** Enter formula. If none, leave box blank: \[ \text{[Box]} \]3. **Which species acts as a reaction intermediate?** Enter formula. If none, leave box blank: \[ \text{[Box]} \]4. **Complete the rate law for the overall reaction that is consistent with this mechanism.** *(Use the form \( k[\text{A}]^m[\text{B}]^n \ldots \), where '1' is understood (so don't write it) for \( m, n \) etc.)* \[ \text{Rate} = \text{[Box]} \]

Answered: One possible mechanism for the gas…

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...

See similar textbooks

Related questions

Question

# Gas Phase Reaction Mechanism

One possible mechanism for the gas phase reaction of hydrogen with nitrogen monoxide is:

### Step 1: (Slow)
\[ \text{H}_2(g) + 2 \text{NO}(g) \rightarrow \text{N}_2\text{O}(g) + \text{H}_2\text{O}(g) \]

### Step 2: (Fast)
\[ \text{N}_2\text{O}(g) + \text{H}_2(g) \rightarrow \text{N}_2(g) + \text{H}_2\text{O}(g) \]

## Questions

1. **What is the equation for the overall reaction?**
Use the smallest integer coefficients possible. If a box is not needed, leave it blank.

\[ \text{[Box]} + \text{[Box]} \rightarrow \text{[Box]} + \text{[Box]} \]

2. **Which species acts as a catalyst?**
Enter formula. If none, leave box blank: \[ \text{[Box]} \]

3. **Which species acts as a reaction intermediate?**
Enter formula. If none, leave box blank: \[ \text{[Box]} \]

4. **Complete the rate law for the overall reaction that is consistent with this mechanism.**

*(Use the form \( k[\text{A}]^m[\text{B}]^n \ldots \), where '1' is understood (so don't write it) for \( m, n \) etc.)*

\[ \text{Rate} = \text{[Box]} \]

Expert Solution

Step 1 Theory

Rate of reaction is given by the slowest step.

Rate law expression must not contain any intermediate species.

Catalyst is a substance which increases the rate of reaction without itself getting consumed during reaction. Catalyst regenerated after the reaction.

Intermediate are species which are produced during the reaction. They do not exist independently.

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions