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 200. mL flask with 2.6 atm of sulfur dioxide gas and 0.90 atm of oxygen gas at 35.°C. She then raises the temperature, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 1.3 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits.

Answer 1

Answer:

Explanation:

By the Application of the ICE -Table to get the pressure equilibrium constant as is carefully analysed and shown in the attached file.

Answer 2

Answer:

The answer is 2.206 × $10^{-1}$ = 0.22 to 2 sig. fig.

Explanation:

Balanced reaction for the equation: y SO2(g) + xO2(g) ⇄ z SO3(g) (where x, y, z are number of moles of reactants and products.

2 SO2(g) + O2(g) ⇄ 2 SO3(g)

Pressure equilibrium constant, Kp = $\frac{(Press SO3)^z}{(Press SO2)^y + (Press O2)^z}$

Kp = $1.3^{2}$ ÷ ($2.6^{2}$ + 0.9)

= $\frac{1.69}{7.66}$

∴ Kp = 2.206 × $10^{-1}$