Question

sulfur trioxide decomposes to form sulfur dioxide and oxygen, like this:

$2so_{3}(g)\to2so_{2}(g)+o_{2}(g)$

also, a chemist finds that at a certain temperature the equilibrium mixture of sulfur trioxide, sulfur dioxide, and oxygen has the following composition:

calculate the value of the equilibrium constant $k_{p}$ for this reaction. round your answer to 2 significant digits.

$k_{p}=\square$

Explanation:

Step1: Write the formula for \(K_p\)

For the reaction \(2SO_3(g)\to2SO_2(g)+O_2(g)\), the formula for \(K_p\) is \(K_p=\frac{P_{SO_2}^2\times P_{O_2}}{P_{SO_3}^2}\)

Step2: Substitute the values

Substitute \(P_{SO_3} = 73.6\ atm\), \(P_{SO_2}=79.5\ atm\), and \(P_{O_2} = 37.4\ atm\) into the formula:

$$
LATEXBLOCK0
$$

Answer:

\(44\)