MnS + H+ < -- > Mn2+ + HS- CuS + H+ < -- > Cu2+ + HS- [A] Classify each reaction as exothermic or endothermic based on the DGr0 (Gibbs energy in kJ/mol). [B] What is the Ksp of MnS and CuS? [C] Which is more soluble? Gibbs free energy given in kJ/mol: CuS = −86.2 MnS = 30
MnS + H+ < -- > Mn2+ + HS- CuS + H+ < -- > Cu2+ + HS- [A] Classify each reaction as exothermic or endothermic based on the DGr0 (Gibbs energy in kJ/mol). [B] What is the Ksp of MnS and CuS? [C] Which is more soluble? Gibbs free energy given in kJ/mol: CuS = −86.2 MnS = 30
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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Given:
MnS + H+ < -- > Mn2+ + HS-
CuS + H+ < -- > Cu2+ + HS-
[A] Classify each reaction as exothermic or endothermic based on the DGr0 (Gibbs energy in kJ/mol).
[B] What is the Ksp of MnS and CuS?
[C] Which is more soluble?
Gibbs free energy given in kJ/mol:
CuS = −86.2
MnS = 30
![### Chemical Reactions
The following are examples of chemical reactions involving metal sulfides and hydrogen ions:
1. **Reaction of Manganese(II) Sulfide:**
\[
\text{MnS} + \text{H}^+ \leftrightarrow \text{Mn}^{2+} + \text{HS}^-
\]
In this reaction, manganese(II) sulfide (MnS) reacts with hydrogen ions (H⁺) to form manganese ions (Mn²⁺) and hydrogen sulfide ions (HS⁻).
2. **Reaction of Copper(II) Sulfide:**
\[
\text{CuS} + \text{H}^+ \leftrightarrow \text{Cu}^{2+} + \text{HS}^-
\]
In this reaction, copper(II) sulfide (CuS) reacts with hydrogen ions (H⁺) to form copper ions (Cu²⁺) and hydrogen sulfide ions (HS⁻).
These reactions are equilibria, indicated by the double arrows (\(\leftrightarrow\)), meaning they can proceed in both forward and reverse directions under certain conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F50bf679e-c229-490b-91d0-8a5b8f84bb57%2Ff146e04a-d6a9-4e7e-87b8-101c7faaebdf%2Fkc4mwjo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Reactions
The following are examples of chemical reactions involving metal sulfides and hydrogen ions:
1. **Reaction of Manganese(II) Sulfide:**
\[
\text{MnS} + \text{H}^+ \leftrightarrow \text{Mn}^{2+} + \text{HS}^-
\]
In this reaction, manganese(II) sulfide (MnS) reacts with hydrogen ions (H⁺) to form manganese ions (Mn²⁺) and hydrogen sulfide ions (HS⁻).
2. **Reaction of Copper(II) Sulfide:**
\[
\text{CuS} + \text{H}^+ \leftrightarrow \text{Cu}^{2+} + \text{HS}^-
\]
In this reaction, copper(II) sulfide (CuS) reacts with hydrogen ions (H⁺) to form copper ions (Cu²⁺) and hydrogen sulfide ions (HS⁻).
These reactions are equilibria, indicated by the double arrows (\(\leftrightarrow\)), meaning they can proceed in both forward and reverse directions under certain conditions.
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