Some SO3 is placed in a flask and heated to 1260 K. When equilibrium is reached, the flask is found to contain SO3 (1.32×10-2 M), SO2 (2.53×10-2 M), and O2 (4.41×10-2 M). What is the value of the equilibrium constant for the following at reaction at 1260 K?

2SO3(g) 2SO2(g) + O2(g)         K = 

To calculate the equilibrium constant \( K \) for the reaction:

\[
2 \, \text{SO}_3 (g) \rightleftharpoons 2 \, \text{SO}_2 (g) + \text{O}_2 (g)
\]

we use the expression for the equilibrium constant in terms of concentrations:

\[
K_c = \frac{[\text{SO}_2]^2 [\text{O}_2]}{[\text{SO}_3]^2}
\]

Given:
- \([\text{SO}_3] = 1.32 \times 10^{-2} \, \text{M}\)
- \([\text{SO}_2] = 2.53 \times 10^{-2} \, \text{M}\)
- \([\text{O}_2] = 4.41 \times 10^{-2} \, \text{M}\)

Now, let's calculate \( K_c \) by substituting these values into the formula.

\[
K_c = \frac{(2.53 \times 10^{-2})^2 \times (4.41 \times 10^{-2})}{(1.32 \times 10^{-2})^2}
\]

I'll compute this for you.The equilibrium constant \( K_c \) for the reaction at 1260 K is approximately \( 0.162 \).

Would you like any further details or clarifications? Here are 5 related questions to deepen your understanding:

1. How is the equilibrium constant affected by temperature?
2. What is the difference between \( K_c \) and \( K_p \) in equilibrium expressions?
3. How does Le Chatelier's Principle apply to this reaction?
4. Why do we square the concentrations of \( \text{SO}_2 \) and \( \text{SO}_3 \) in the \( K_c \) expression?
5. How can the equilibrium constant be used to predict the extent of a reaction?

**Tip:** The value of the equilibrium constant \( K_c \) indicates whether reactants or products are favored at equilibrium; a small value means reactants are favored, while a large value means products are favored.

Some SO3 is placed in a flask and heated to 1260 K. When equilibrium is reached, the flask is found to contain SO3 (1.32×10^-2 M), SO2 (2.53×10^-2 M), and O2 (4.41×10^-2 M). What is the value of the equilibrium constant for the following reaction at 1260 K?

2SO3(g) → 2SO2(g) + O2(g)         K = 

Learn how to calculate the equilibrium constant for the decomposition of SO3 into SO2 and O2 at 1260 K. The solution includes key chemistry concepts such as chemical equilibrium, equilibrium constants, and stoichiometry. Suitable for undergraduate chemistry students.

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