▾ Part B What is the numerical value of K, for the reaction if the concentrations at equilibrium are [SO₂] = 0.15 M. [0₂] = 0.15 M, and [SO3] = 0.57 M? Express your answer using two significant figures. K₂= ΨΕΙ ΑΣΦ ?
▾ Part B What is the numerical value of K, for the reaction if the concentrations at equilibrium are [SO₂] = 0.15 M. [0₂] = 0.15 M, and [SO3] = 0.57 M? Express your answer using two significant figures. K₂= ΨΕΙ ΑΣΦ ?
Chemistry
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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
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![**Equilibrium Constant Expression for a Chemical Reaction**
Consider the following reaction:
\[ 2\text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{SO}_3(g) \]
**Equilibrium Constant Expressions:**
Options for the equilibrium constant (\( K_c \)) expression based on the reaction are:
1. \[ K_c = \frac{[\text{SO}_3]^2}{[\text{O}_2][\text{SO}_2]^2} \] (Selected)
2. \[ K_c = \frac{[\text{O}_2][\text{SO}_2]}{[\text{SO}_3]} \]
3. \[ K_c = \frac{[2\text{SO}_3]}{[\text{O}_2][2\text{SO}_2]} \]
The correct expression is the first one, where the product concentrations are in the numerator, and the reactant concentrations are in the denominator. Each concentration is raised to the power of its stoichiometric coefficient.
**Explanation:**
In the equilibrium-constant expression, the concentrations are multiplicative, so the coefficients from the balanced chemical equation become exponents for the respective concentrations.
Now, use this expression to calculate the equilibrium constant using the equilibrium concentrations of the reactants and product.
**Part B: Calculation of \( K_c \)**
What is the numerical value of \( K_c \) for the reaction if the concentrations at equilibrium are \([\text{SO}_2] = 0.15 \, M\), \([\text{O}_2] = 0.15 \, M\), and \([\text{SO}_3] = 0.57 \, M\)?
*Express your answer using two significant figures.*
\[ K_c = \frac{[\text{SO}_3]^2}{[\text{O}_2][\text{SO}_2]^2} \]
*Insert your calculated value here.*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F59c9f849-9820-4119-beb6-2f585a7a222b%2Fb2f1b070-4dba-4bcb-8069-eff826e21c0f%2Fbludzht_processed.png&w=3840&q=75)
Transcribed Image Text:**Equilibrium Constant Expression for a Chemical Reaction**
Consider the following reaction:
\[ 2\text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{SO}_3(g) \]
**Equilibrium Constant Expressions:**
Options for the equilibrium constant (\( K_c \)) expression based on the reaction are:
1. \[ K_c = \frac{[\text{SO}_3]^2}{[\text{O}_2][\text{SO}_2]^2} \] (Selected)
2. \[ K_c = \frac{[\text{O}_2][\text{SO}_2]}{[\text{SO}_3]} \]
3. \[ K_c = \frac{[2\text{SO}_3]}{[\text{O}_2][2\text{SO}_2]} \]
The correct expression is the first one, where the product concentrations are in the numerator, and the reactant concentrations are in the denominator. Each concentration is raised to the power of its stoichiometric coefficient.
**Explanation:**
In the equilibrium-constant expression, the concentrations are multiplicative, so the coefficients from the balanced chemical equation become exponents for the respective concentrations.
Now, use this expression to calculate the equilibrium constant using the equilibrium concentrations of the reactants and product.
**Part B: Calculation of \( K_c \)**
What is the numerical value of \( K_c \) for the reaction if the concentrations at equilibrium are \([\text{SO}_2] = 0.15 \, M\), \([\text{O}_2] = 0.15 \, M\), and \([\text{SO}_3] = 0.57 \, M\)?
*Express your answer using two significant figures.*
\[ K_c = \frac{[\text{SO}_3]^2}{[\text{O}_2][\text{SO}_2]^2} \]
*Insert your calculated value here.*
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