The formation constants at 25°C for Fe(CN)64– and Fe(EDTA)2– are 1.00x1037 and 2.10x1014, respectively. Calculate K under standard conditions for the reaction. Calculate ΔG° for the reaction.
The formation constants at 25°C for Fe(CN)64– and Fe(EDTA)2– are 1.00x1037 and 2.10x1014, respectively. Calculate K under standard conditions for the reaction. Calculate ΔG° for the reaction.
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...
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The formation constants at 25°C for Fe(CN)64– and Fe(EDTA)2– are 1.00x1037 and 2.10x1014, respectively.
Calculate K under standard conditions for the reaction.
Calculate ΔG° for the reaction.
![The chemical equation depicted is as follows:
\[ \text{Fe(EDTA)}^{2-} \, (aq) + 6 \, \text{CN}^- \, (aq) \leftrightarrow \text{Fe(CN)}_6^{4-} \, (aq) + \text{EDTA}^{4-} \, (aq) \]
This equation represents a reversible reaction in an aqueous solution where a complex ion of iron and ethylenediaminetetraacetate (EDTA) reacts with cyanide ions. The reaction results in the formation of a hexacyanoferrate(II) ion and free EDTA.
Key points:
- \(\text{Fe(EDTA)}^{2-} (aq)\) is a complex ion of iron and EDTA.
- \(\text{CN}^- (aq)\) represents cyanide ions in solution.
- \(\text{Fe(CN)}_6^{4-} (aq)\) is a hexacyanoferrate(II) ion.
- \(\text{EDTA}^{4-} (aq)\) denotes the free EDTA ligand in its tetravalent anion form.
- The reaction is reversible, indicated by the double arrow (\(\leftrightarrow\)).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fddc1ec45-98e4-4675-b97b-277ce49cbbd0%2Ff399f9ac-ce3c-46c5-8292-abb89af1c439%2Fn8750c_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The chemical equation depicted is as follows:
\[ \text{Fe(EDTA)}^{2-} \, (aq) + 6 \, \text{CN}^- \, (aq) \leftrightarrow \text{Fe(CN)}_6^{4-} \, (aq) + \text{EDTA}^{4-} \, (aq) \]
This equation represents a reversible reaction in an aqueous solution where a complex ion of iron and ethylenediaminetetraacetate (EDTA) reacts with cyanide ions. The reaction results in the formation of a hexacyanoferrate(II) ion and free EDTA.
Key points:
- \(\text{Fe(EDTA)}^{2-} (aq)\) is a complex ion of iron and EDTA.
- \(\text{CN}^- (aq)\) represents cyanide ions in solution.
- \(\text{Fe(CN)}_6^{4-} (aq)\) is a hexacyanoferrate(II) ion.
- \(\text{EDTA}^{4-} (aq)\) denotes the free EDTA ligand in its tetravalent anion form.
- The reaction is reversible, indicated by the double arrow (\(\leftrightarrow\)).
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