The equilibrium concentrations for the reaction between [tex]SO_2[/tex] and [tex]O_2[/tex] to form [tex]SO_3[/tex] at a certain temperature are given in the table below. Determine the equilibrium constant and whether the reaction favors reactants, products, or neither at this temperature.

[tex]\[ O_2(g) + 2SO_2(g) \rightleftharpoons 2SO_3(g) \][/tex]

\begin{tabular}{|l|l|l|}
\hline
\multicolumn{1}{|c|}{[tex]$[O_2]$[/tex]} & \multicolumn{1}{c|}{[tex]$[SO_2]$[/tex]} & \multicolumn{1}{c|}{[tex]$[SO_3]$[/tex]} \\
\hline
1.2 M & 0.80 M & 1.9 M \\
\hline
\end{tabular}

A. [tex]K=4.7[/tex]; product favored
B. [tex]K=0.51[/tex]; product favored
C. [tex]K=0.51[/tex]; reactant favored
D. [tex]K=4.7[/tex]; reactant favored



Answer :

To solve this problem, we need to determine the equilibrium constant ([tex]\(K\)[/tex]) for the given reaction:

[tex]\[O_2(g) + 2SO_2(g) \rightleftarrows 2SO_3(g)\][/tex]

The equilibrium expression for this reaction is given as:

[tex]\[ K = \frac{[SO_3]^2}{[O_2] \cdot [SO_2]^2} \][/tex]

Given the equilibrium concentrations from the table:

[tex]\[ [O_2] = 1.2 \, \text{M} \][/tex]
[tex]\[ [SO_2] = 0.80 \, \text{M} \][/tex]
[tex]\[ [SO_3] = 1.9 \, \text{M} \][/tex]

We can substitute these values into the equilibrium expression to calculate [tex]\( K \)[/tex]:

[tex]\[ K = \frac{[SO_3]^2}{[O_2] \cdot [SO_2]^2} \][/tex]

[tex]\[ K = \frac{(1.9)^2}{1.2 \cdot (0.80)^2} \][/tex]

Calculating the squares and products in the denominator and numerator:

[tex]\[ (1.9)^2 = 3.61 \][/tex]
[tex]\[ (0.80)^2 = 0.64 \][/tex]
[tex]\[ 1.2 \cdot 0.64 = 0.768 \][/tex]

Now, divide the results:

[tex]\[ K = \frac{3.61}{0.768} \approx 4.700520833333332 \][/tex]

Now that we have the value of [tex]\(K\)[/tex], we determine whether the reaction favors the reactants or the products by comparing the value of [tex]\(K\)[/tex] with 1.

- If [tex]\(K > 1\)[/tex], the reaction favors the formation of products.
- If [tex]\(K < 1\)[/tex], the reaction favors the formation of reactants.

In this case, [tex]\(K \approx 4.7\)[/tex], which is greater than 1, indicating that the reaction favors the formation of products.

Now, we review the answer choices:

A. [tex]\(K = 4.7\)[/tex]; product favored
B. [tex]\(K = 0.51\)[/tex]; product favored
C. [tex]\(K = 0.51\)[/tex]; reactant favored
D. [tex]\(K = 4.7\)[/tex]; reactant favored

Given our calculated [tex]\(K\)[/tex] value of approximately 4.7 and the understanding that this [tex]\(K\)[/tex] value indicates a product-favored reaction, the closest match in the provided choices would ideally be choice A. However, none of the given answer choices exactly match our findings in both [tex]\(K\)[/tex] value and description.

Thus, the final numerical result and determination is:

[tex]\[ K \approx 4.700520833333332, \quad \text{product favored}, \quad \text{None of the provided choices exactly match.} \][/tex]