The reaction has an equilibrium constant of = 0.154. If 6.60 of , 4.30 of , and 11.60 of are added to a reaction vessel with a volume of 5.30 , what net reaction will occur?
A-The reaction will proceed to the left to establish equilibrium. B-The reaction will proceed to the right to establish equilibrium. C-No further reaction will occur because the reaction is at equilibrium.
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To determine the net reaction that will occur, we need to compare the initial concentrations of the reactants to the equilibrium constant.
Given:
[NO₂] = 6.60 mol / 5.30 L = 1.245 M
[CO] = 4.30 mol / 5.30 L = 0.811 M
[NO] = 11.60 mol / 5.30 L = 2.189 M
Kc = 0.154
Let's write the balanced chemical equation for the reaction:
2NO₂(g) + CO(g) ⇌ 2NO(g) + CO₂(g)
Now, let's compare the initial concentrations to the equilibrium constant using the reaction quotient, Qc:
Qc = ([NO]² * [CO₂]) / ([NO₂]² * [CO])
Substituting the given values:
Qc = (2.189² * [CO₂]) / (1.245² * 0.811)
Since we don't know the concentration of CO₂, we cannot calculate the exact value of Qc. However, we can compare Qc to Kc to determine the direction of the net reaction.
If Qc < Kc, the reaction will proceed to the right to establish equilibrium (Option B).
If Qc > Kc, the reaction will proceed to the left to establish equilibrium (Option A).
If Qc = Kc, no further reaction will occur because the reaction is already at equilibrium (Option C).
Therefore, to determine the net reaction that will occur, you need to calculate Qc and compare it to Kc to choose the appropriate option.