Fe²+ + O2(eq) + H+ (eq) eq AG°f=(Fe²+eq = -78.87),( 02(eq) = 16.32),( H+ Will the forward rxn occur? Step 1: balance the reaction. Step 2 calculate AG° = -RT ln k {C}{D}d {A}{B}b. Step 3 calculate k = Step 4 calculate Q mg If there is 0.001 M of Fe2+, 0.002M of Fe³+,8- of 02. And 10-7M of H+. L = = (eq) {C} c{D}d {A}a{B}b Step. 5 compare K and Q. using AG -RT ln k. Alternative: step 3: Calculate AG using AG = AG° + RT ln Q → Fe³+ eq + H₂0 (1) eq = -4.60), (H₂0 (1) = -237.18) 0),( Fe³+
Fe²+ + O2(eq) + H+ (eq) eq AG°f=(Fe²+eq = -78.87),( 02(eq) = 16.32),( H+ Will the forward rxn occur? Step 1: balance the reaction. Step 2 calculate AG° = -RT ln k {C}{D}d {A}{B}b. Step 3 calculate k = Step 4 calculate Q mg If there is 0.001 M of Fe2+, 0.002M of Fe³+,8- of 02. And 10-7M of H+. L = = (eq) {C} c{D}d {A}a{B}b Step. 5 compare K and Q. using AG -RT ln k. Alternative: step 3: Calculate AG using AG = AG° + RT ln Q → Fe³+ eq + H₂0 (1) eq = -4.60), (H₂0 (1) = -237.18) 0),( Fe³+
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
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I want you to give me step by step solution and describe everything.
![### Chemical Reaction and Equilibrium Analysis
**Reaction:**
\[ \text{Fe}^{2+}_{(aq)} + \text{O}_2{(aq)} + \text{H}^+_{(aq)} \rightarrow \text{Fe}^{3+}_{(aq)} + \text{H}_2\text{O}_{(l)} \]
**Standard Gibbs Free Energy of Formation:**
- \( \Delta G^\circ_f = (\text{Fe}^{2+}_{(aq)} = -78.87), (\text{O}_2{(aq)} = 16.32), (\text{H}^+_{(aq)} = 0), (\text{Fe}^{3+}_{(aq)} = -4.60), (\text{H}_2\text{O}_{(l)} = -237.18) \)
**Conditions:**
- Concentration of \(\text{Fe}^{2+}\): 0.001 M
- Concentration of \(\text{Fe}^{3+}\): 0.002 M
- Concentration of \(\text{O}_2\): 8 mg/L
- Concentration of \(\text{H}^+\): \(10^{-7}\) M
**Question:**
Will the forward reaction occur?
**Procedure:**
**Step 1:** Balance the reaction.
**Step 2:** Calculate \(\Delta G^\circ\) using:
\[ \Delta G^\circ = -RT \ln k \]
**Step 3:** Calculate the equilibrium constant \(k\):
\[ k = \frac{ \{ C \}^c \{ D \}^d }{ \{ A \}^a \{ B \}^b } \]
**Step 4:** Calculate the reaction quotient \(Q\):
\[ Q = \frac{ \{ C \}^c \{ D \}^d }{ \{ A \}^a \{ B \}^b } \]
**Step 5:** Compare \(K\) and \(Q\).
**Using Equation:**
\[ \Delta G^\circ = -RT \ln k \]
**Alternative Approach:**
**Step 3:** Calculate \(\Delta G\) using:
\[ \Delta G = \Delta G^\circ + RT \ln Q \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4ce8b870-93ef-497a-8c2a-bbbd1041dd5b%2Fb3de633b-5919-4c12-b61d-d86dfad43203%2Fpvm4q1p_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Reaction and Equilibrium Analysis
**Reaction:**
\[ \text{Fe}^{2+}_{(aq)} + \text{O}_2{(aq)} + \text{H}^+_{(aq)} \rightarrow \text{Fe}^{3+}_{(aq)} + \text{H}_2\text{O}_{(l)} \]
**Standard Gibbs Free Energy of Formation:**
- \( \Delta G^\circ_f = (\text{Fe}^{2+}_{(aq)} = -78.87), (\text{O}_2{(aq)} = 16.32), (\text{H}^+_{(aq)} = 0), (\text{Fe}^{3+}_{(aq)} = -4.60), (\text{H}_2\text{O}_{(l)} = -237.18) \)
**Conditions:**
- Concentration of \(\text{Fe}^{2+}\): 0.001 M
- Concentration of \(\text{Fe}^{3+}\): 0.002 M
- Concentration of \(\text{O}_2\): 8 mg/L
- Concentration of \(\text{H}^+\): \(10^{-7}\) M
**Question:**
Will the forward reaction occur?
**Procedure:**
**Step 1:** Balance the reaction.
**Step 2:** Calculate \(\Delta G^\circ\) using:
\[ \Delta G^\circ = -RT \ln k \]
**Step 3:** Calculate the equilibrium constant \(k\):
\[ k = \frac{ \{ C \}^c \{ D \}^d }{ \{ A \}^a \{ B \}^b } \]
**Step 4:** Calculate the reaction quotient \(Q\):
\[ Q = \frac{ \{ C \}^c \{ D \}^d }{ \{ A \}^a \{ B \}^b } \]
**Step 5:** Compare \(K\) and \(Q\).
**Using Equation:**
\[ \Delta G^\circ = -RT \ln k \]
**Alternative Approach:**
**Step 3:** Calculate \(\Delta G\) using:
\[ \Delta G = \Delta G^\circ + RT \ln Q \]
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