Question

Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a flask with of sulfur dioxide gas and of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be . Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to significant digits.

Answer 1

The answer is "
`\bold{4.97 * 10^(-2)}`"

Step-by-step explanation:

Please find the complete question in the attached file.

Equation:

`2SO_2+O_2 \leftrightharpoons 2SO_3`

at
`t=0 3.3 \ \ \ \ \ \ \ \ \ \ 0.79`

at equilibrium
`3.3-p \ \ \ \ \ \ \ \ \ \ 0.79 - (P)/(2) \ \ \ \ \ \ \ \ \ \ \ \ P`

`p= 0.47 \ \ atm\\\\SO_2=3.3-0.47 = 2.83 \ \ atm\\\\O_2= 0.74 -(0.47)/(2)=0.74-0.235=0.555 \ atm\\\\K_P=([PSO_3]^2)/([PSO_2]^2[PO_2])\\\\`

`=(0.47^2)/(2.83^2* 0.555)\\\\=4.97 * 10^(-2)`