Homework Help is Here – Start Your Trial Now!
Science
Chemistry
For the equilibrium A+B=C+D K was measured to be 1.20 at 25 °C and 1.15 x 10² at 300 °C. What is AH° for the reaction?

For the equilibrium A+B=C+D K was measured to be 1.20 at 25 °C and 1.15 x 10² at 300 °C. What is AH° for the reaction?

Chemistry
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
icon
Related questions
Question

Please don't provide hand written solution.....

 

**Equilibrium Constant and Enthalpy Change** For the equilibrium reaction: \[ \text{A} + \text{B} \rightleftharpoons \text{C} + \text{D} \] The equilibrium constant (\( K \)) was measured to be 1.20 at 25 °C and \( 1.15 \times 10^{-2} \) at 300 °C. Determine \( \Delta H^\circ \) for the reaction. --- **Understanding the Reaction Parameters:** - **Equilibrium Constant (\( K \))**: This value indicates the ratio of the concentration of products to reactants at equilibrium. A larger \( K \) favors products, while a smaller \( K \) favors reactants. - **Temperature Influence on \( K \)**: Changes in temperature can shift the equilibrium position, affecting \( K \). In this scenario, observe how \( K \) changes from a higher value at a lower temperature to a significantly smaller value at a higher temperature. - **Enthalpy Change (\( \Delta H^\circ \))**: This is the heat absorbed or released during a reaction at constant pressure. It can be determined using the van 't Hoff equation, which relates the change in \( K \) over temperature to \( \Delta H^\circ \).
Transcribed Image Text:**Equilibrium Constant and Enthalpy Change** For the equilibrium reaction: \[ \text{A} + \text{B} \rightleftharpoons \text{C} + \text{D} \] The equilibrium constant (\( K \)) was measured to be 1.20 at 25 °C and \( 1.15 \times 10^{-2} \) at 300 °C. Determine \( \Delta H^\circ \) for the reaction. --- **Understanding the Reaction Parameters:** - **Equilibrium Constant (\( K \))**: This value indicates the ratio of the concentration of products to reactants at equilibrium. A larger \( K \) favors products, while a smaller \( K \) favors reactants. - **Temperature Influence on \( K \)**: Changes in temperature can shift the equilibrium position, affecting \( K \). In this scenario, observe how \( K \) changes from a higher value at a lower temperature to a significantly smaller value at a higher temperature. - **Enthalpy Change (\( \Delta H^\circ \))**: This is the heat absorbed or released during a reaction at constant pressure. It can be determined using the van 't Hoff equation, which relates the change in \( K \) over temperature to \( \Delta H^\circ \).
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 7 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Thermodynamics
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
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
SEE MORE TEXTBOOKS