At a certain temperature, the reaction below has an equilibrium constant of 420.
ID: 712962 • Letter: A
Question
At a certain temperature, the reaction below has an equilibrium constant of 420. Which of the following is correct if 3.4 moles of sulfur trioxide, 1.2 moles of sulfur dioxide, and 2.8 moles of oxygen are placed
in an 8.4 L container and allowed to reach equilibrium at this temperature?
2 SO3 (g) 2 SO2 (g) + O2 (g)
Q = 3.0 and the system reaches equilibrium by increasing the amount of SO3.
Q = 0.042 and the system reaches equilibrium by decreasing the amount of SO3.
Q = 0.35 and the system reaches equilibrium by increasing the amount of SO3.
Q = 0.042 and the system reaches equilibrium by increasing the amount of SO3.
Q = 0.35 and the system reaches equilibrium by decreasing the amount of SO3.
Q = 3.0 and the system reaches equilibrium by increasing the amount of SO3.
Q = 0.042 and the system reaches equilibrium by decreasing the amount of SO3.
Q = 0.35 and the system reaches equilibrium by increasing the amount of SO3.
Q = 0.042 and the system reaches equilibrium by increasing the amount of SO3.
Q = 0.35 and the system reaches equilibrium by decreasing the amount of SO3.
Explanation / Answer
2SO3(g) <--> 2SO2(g) + O2(g)
Q = [SO2]2*[O2]/[SO3]2
Q = 1.22*2.8/3.42
Q = 0.35
And as per le chatelier's principle, increasing the amount of reactant, shifts the reaction towards equilibrium.
Option C
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