Use the References to access important values if needed for this question. The gas phase reaction of hydrogen with iodine H2 + I 2 HI is first order in H, and first order in I,. Complete the rate law for this reaction in the box below. Use the form k[A]"|B]"... , where 'l' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 5.71×10-21 Ms- when [H,]= 9.26×10-² M and [I,] = 2.60×10² M. From this experiment, the rate constant is Mls1.

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...
icon
Related questions
Question
100%
**The Gas Phase Reaction of Hydrogen with Iodine**

The chemical reaction is represented as:

\[ \textbf{H}_2 + \textbf{I}_2 \rightarrow 2 \textbf{HI} \]

This reaction is **first order** in \(\textbf{H}_2\) and **first order** in \(\textbf{I}_2\).

**Complete the Rate Law**

To establish the rate law for this reaction, use the form \( k[\text{A}]^m[\text{B}]^n \), where '1' is understood for \( m \) and \( n \). Concentrations taken to the zero power do not appear.

\[ \text{Rate} = \underline{\hspace{4cm}} \]

**Experimental Determination of the Rate Law**

In an experiment to evaluate the rate law, the reaction rate was found to be \( 5.71 \times 10^{-21} \, \text{M/s}^{-1} \) when \([\text{H}_2] = 9.26 \times 10^{-2} \, \text{M} \) and \([\text{I}_2] = 2.60 \times 10^{-2} \, \text{M} \). From this experiment, the rate constant is:

\[ \underline{\hspace{2cm}} \, \text{M}^{-1}\text{s}^{-1} \]
Transcribed Image Text:**The Gas Phase Reaction of Hydrogen with Iodine** The chemical reaction is represented as: \[ \textbf{H}_2 + \textbf{I}_2 \rightarrow 2 \textbf{HI} \] This reaction is **first order** in \(\textbf{H}_2\) and **first order** in \(\textbf{I}_2\). **Complete the Rate Law** To establish the rate law for this reaction, use the form \( k[\text{A}]^m[\text{B}]^n \), where '1' is understood for \( m \) and \( n \). Concentrations taken to the zero power do not appear. \[ \text{Rate} = \underline{\hspace{4cm}} \] **Experimental Determination of the Rate Law** In an experiment to evaluate the rate law, the reaction rate was found to be \( 5.71 \times 10^{-21} \, \text{M/s}^{-1} \) when \([\text{H}_2] = 9.26 \times 10^{-2} \, \text{M} \) and \([\text{I}_2] = 2.60 \times 10^{-2} \, \text{M} \). From this experiment, the rate constant is: \[ \underline{\hspace{2cm}} \, \text{M}^{-1}\text{s}^{-1} \]
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 2 images

Blurred answer
Knowledge Booster
Rate Laws
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
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY