Consider the following reaction where K_c = 2.90 times 10^-2 at 1150 K: 2 SO_3 (
ID: 487628 • Letter: C
Question
Consider the following reaction where K_c = 2.90 times 10^-2 at 1150 K: 2 SO_3 (g) 2 SO_2 (g) + O_2 (g) A reaction mixture was found to contain 4.19 times 10^-2 moles of SO_3 (g), 4.91 times 10^2 moles of SO_2 (g), and 3.89 times 10^-2 moles of O_2 (g), in a 1.00 liter container. Indicate True (T) or False (F) for each of the following. In order to reach equilibrium SO_3 (g) must be produced In order to reach equilibrium K_C must decrease. In order to reach equilibrium SO_2 must be produced. Q_C is greater than K_C.Explanation / Answer
First
calculate Q
Q = [SO2]^2[O2] / [SO3]^2
compare Q vs. Kc
so
Q = (4.91*10^-2)^2(3.89*10^-2) / (4.19*10^-2)^2
Q = 0.053417 = 5.3*10^-2
since
Q > Kc
the equilibrium will shift toward more SO3, in order to Q = K
1. SO3 must be produced, in order to lower Q value, this is TRUE
2. Kc cant increase since it is constant at T constant, False
3. SO2 must decrease, so this is False
4. Qc > Kc si true
Q5. The reaction is NOT at equilibrium since Qc is not Kc