calculate the change in gibbs free energy in kJ for the reaction below at 7l0.4°C when there is a pressure Of. O548atm Hz, o235atm Clz and 7.48atm Hl. For Hulg), AO$= -95.3K7/md.

Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
icon
Related questions
Question
**Topic: Calculating Gibbs Free Energy Change**

**Objective:**
Learn how to calculate the change in Gibbs free energy for a chemical reaction using given conditions of temperature and pressure.

**Problem Statement:**
Calculate the change in Gibbs free energy \( \Delta G \) in kJ for the reaction below at 715°C when there is a pressure of 1.235 atm \( O_2 \) and 0.9548 atm \( H_2 \):

\[ 2H_2 (g) + O_2 (g) \leftrightarrow 2H_2O (g) \]

Given data:
- Standard Gibbs free energy change \( \Delta G^0 \) for \( H_2O(g) \) = -9.53 kJ/mol 

**Explanation:**
This problem requires the application of thermodynamic principles to determine the Gibbs free energy change. 

**Step-by-step Solution:**

1. **Write down the reaction:**

   \[ 2H_2 (g) + O_2 (g) \leftrightarrow 2H_2O (g) \]

2. **Use the given standard Gibbs free energy change for water in its gaseous form:**

   \[ \Delta G^0_{H2O(g)} = -9.53 \text{ kJ/mol} \]

3. **Convert the temperature from Celsius to Kelvin:**

   \[ T(K) = 715°C + 273.15 = 988.15 \text{ K} \]

4. **Determine the reaction quotient \( Q \):**

   \[ Q = \frac{(\text{Pressure of } H_2O)^2}{(\text{Pressure of } H_2)^2 \times (\text{Pressure of } O_2)} = \frac{(P_{H_2O})^2}{(0.9548 \text{ atm})^2 \times (1.235 \text{ atm})} \]

   Since pressures of water are not given, proceed assuming \( P_{H_2O} \) can be derived or set under standard conditions if unavailable.

5. **Use the Gibbs free energy equation that relates \( \Delta G \) to \( \Delta G^0 \) and \( Q \):**

   \[ \Delta G = \Delta G^0 + RT \ln Q
Transcribed Image Text:**Topic: Calculating Gibbs Free Energy Change** **Objective:** Learn how to calculate the change in Gibbs free energy for a chemical reaction using given conditions of temperature and pressure. **Problem Statement:** Calculate the change in Gibbs free energy \( \Delta G \) in kJ for the reaction below at 715°C when there is a pressure of 1.235 atm \( O_2 \) and 0.9548 atm \( H_2 \): \[ 2H_2 (g) + O_2 (g) \leftrightarrow 2H_2O (g) \] Given data: - Standard Gibbs free energy change \( \Delta G^0 \) for \( H_2O(g) \) = -9.53 kJ/mol **Explanation:** This problem requires the application of thermodynamic principles to determine the Gibbs free energy change. **Step-by-step Solution:** 1. **Write down the reaction:** \[ 2H_2 (g) + O_2 (g) \leftrightarrow 2H_2O (g) \] 2. **Use the given standard Gibbs free energy change for water in its gaseous form:** \[ \Delta G^0_{H2O(g)} = -9.53 \text{ kJ/mol} \] 3. **Convert the temperature from Celsius to Kelvin:** \[ T(K) = 715°C + 273.15 = 988.15 \text{ K} \] 4. **Determine the reaction quotient \( Q \):** \[ Q = \frac{(\text{Pressure of } H_2O)^2}{(\text{Pressure of } H_2)^2 \times (\text{Pressure of } O_2)} = \frac{(P_{H_2O})^2}{(0.9548 \text{ atm})^2 \times (1.235 \text{ atm})} \] Since pressures of water are not given, proceed assuming \( P_{H_2O} \) can be derived or set under standard conditions if unavailable. 5. **Use the Gibbs free energy equation that relates \( \Delta G \) to \( \Delta G^0 \) and \( Q \):** \[ \Delta G = \Delta G^0 + RT \ln Q
Expert Solution
steps

Step by step

Solved in 2 steps with 2 images

Blurred answer
Knowledge Booster
Stoichiometry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemical-engineering and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Introduction to Chemical Engineering Thermodynami…
Introduction to Chemical Engineering Thermodynami…
Chemical Engineering
ISBN:
9781259696527
Author:
J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:
McGraw-Hill Education
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemical Engineering
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
Elements of Chemical Reaction Engineering (5th Ed…
Elements of Chemical Reaction Engineering (5th Ed…
Chemical Engineering
ISBN:
9780133887518
Author:
H. Scott Fogler
Publisher:
Prentice Hall
Process Dynamics and Control, 4e
Process Dynamics and Control, 4e
Chemical Engineering
ISBN:
9781119285915
Author:
Seborg
Publisher:
WILEY
Industrial Plastics: Theory and Applications
Industrial Plastics: Theory and Applications
Chemical Engineering
ISBN:
9781285061238
Author:
Lokensgard, Erik
Publisher:
Delmar Cengage Learning
Unit Operations of Chemical Engineering
Unit Operations of Chemical Engineering
Chemical Engineering
ISBN:
9780072848236
Author:
Warren McCabe, Julian C. Smith, Peter Harriott
Publisher:
McGraw-Hill Companies, The