For the isomerization reaction:
Butane ⇌ isobutane
K_p equals 25.0 at 500 °C.If the initial pressures of butane and isobutane are 20.0 atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

Question

Quizplus · Accepted Answer

Given the equilibrium constant (K) is 25.0, and the initial pressure of butane is 20.0 atm with isobutane starting at 0.0 atm, the system will shift towards isobutane to reach equilibrium. Using the equilibrium expression $K = \frac{P_{\text{isobutane}}}{P_{\text{butane}}}$ and solving for the pressures at equilibrium, option A provides the correct pressures that align with the given K value, indicating the system has shifted towards isobutane, increasing its pressure while decreasing the pressure of butane.

For the Isomerization Reaction