Answer:
The system is not at equilibrium and the reaction will shift to the right until Kp = Q
Explanation:
For the reaction:
cis-2-butene ⇌ trans-2-butene
Kp is defined as:
[tex]Kp = 3.40 = \frac{P_{trans-2-butene}}{P_{cis-2-butene}}[/tex]
Where P is the pressure of each gas in equilibrium.
If initially, a flask contains 5.00atm of each gas, Q of reaction will be:
Q = 5.00 atm / 5.00 atm = 1.
As Kp > Q, the system is not at equilibrium and the reaction will shift to the right until Kp = Q
