Question

sulfuric acid has many uses, making it the most produced chemical in the world (over 150 million tons a year). one of the steps in the manufacture of sulfuric acid is so2(g) 1/2 o2(g) equilibrium reaction arrow so3(g). a sealed flask at 627°c is loaded with 1.48 atm of so2 and 0.74 atm of o2. after reaction, the equilibrium pressure of so3 is found to be 1.10 atm. what is the value of kp for this reaction at 627°c?

Answer 1

To find the value of Kp for the given reaction, use the ideal gas law and the equilibrium expression.

Step-by-step explanation:

To find the value of Kp for the given reaction, we can use the ideal gas law and the equilibrium expression. The equilibrium expression for the reaction is:

Kp = (P(SO3))^2 / (P(SO2))^2 * (P(O2))^1/2

Using the given equilibrium pressure values (P(SO3) = 1.10 atm, P(SO2) = 1.48 atm, P(O2) = 0.74 atm), we can substitute them into the equation and solve for Kp.