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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Question
lab2-1: please see attached
![### Equilibrium Expression for the Reaction
**Problem Statement:**
Write the equilibrium expression for the following reaction.
\[ \text{Fe}^{2+} (\text{aq}) + \text{SCN}^{-} (\text{aq}) \rightleftharpoons [\text{FeSCN}]^{+} (\text{aq}) \]
**Answer:**
The equilibrium constant (K) expression for the given reaction is calculated using the concentrations of the products and reactants at equilibrium. For the general reaction:
\[ aA + bB \rightleftharpoons cC + dD \]
The equilibrium constant expression is given by:
\[ K = \frac{[\text{C}]^c [\text{D}]^d}{[\text{A}]^a [\text{B}]^b} \]
For the specific reaction provided, the equilibrium constant expression (K) is:
\[ K = \frac{[\text{FeSCN}]^{+}}{[\text{Fe}^{2+}][\text{SCN}^{-}]} \]
Where:
- \([\text{FeSCN}]^{+}\) is the concentration of the complex ion at equilibrium.
- \([\text{Fe}^{2+}]\) is the concentration of iron(II) ions at equilibrium.
- \([\text{SCN}^{-}]\) is the concentration of thiocyanate ions at equilibrium.
This expression shows the relationship between the concentrations of the reactants and the product when the reaction has reached its equilibrium state.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1dedc2f0-34a2-4f6a-9bbc-fab867b2dfd0%2Fe8ac8698-f7c3-4bbf-b811-cf8f756b0904%2F0u2foqn.png&w=3840&q=75)
Transcribed Image Text:### Equilibrium Expression for the Reaction
**Problem Statement:**
Write the equilibrium expression for the following reaction.
\[ \text{Fe}^{2+} (\text{aq}) + \text{SCN}^{-} (\text{aq}) \rightleftharpoons [\text{FeSCN}]^{+} (\text{aq}) \]
**Answer:**
The equilibrium constant (K) expression for the given reaction is calculated using the concentrations of the products and reactants at equilibrium. For the general reaction:
\[ aA + bB \rightleftharpoons cC + dD \]
The equilibrium constant expression is given by:
\[ K = \frac{[\text{C}]^c [\text{D}]^d}{[\text{A}]^a [\text{B}]^b} \]
For the specific reaction provided, the equilibrium constant expression (K) is:
\[ K = \frac{[\text{FeSCN}]^{+}}{[\text{Fe}^{2+}][\text{SCN}^{-}]} \]
Where:
- \([\text{FeSCN}]^{+}\) is the concentration of the complex ion at equilibrium.
- \([\text{Fe}^{2+}]\) is the concentration of iron(II) ions at equilibrium.
- \([\text{SCN}^{-}]\) is the concentration of thiocyanate ions at equilibrium.
This expression shows the relationship between the concentrations of the reactants and the product when the reaction has reached its equilibrium state.
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