Hi! I kep trying this question and can't get it right. At a certain temperature, the equilibrium...

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Chemistry

Hi!
I kep trying this question and can't get it right.
At a certain temperature, the equilibrium constant for thefollowing chemical equation is 2.90. At this temperature, calculatethe number of moles of NO2(g) that must be added to 2.73 mol ofSO2(g) in order to form 1.30 mol of SO3(g) at equilibrium.
SO2(g) + NO2(g) ----> SO3 (g) + NO (g)
Answer in mol NO2

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4.0 Ratings (597 Votes)

Let number of moles of NO2 to be added be x

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â SO2(g) + NO2(g) ----> SO3 (g) + NO (g)

initial:Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 2.73Â Â Â Â Â Â Â Â Â xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0Â Â Â Â Â Â Â Â Â Â Â Â Â 0

At equilibrium:Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 2.73-yÂ Â Â Â Â Â Â Â x-yÂ Â Â Â Â Â Â Â Â Â Â Â Â yÂ Â Â Â Â Â Â Â Â Â Â Â Â Â y

Given in question that: number of mol of SO3 at equilibrium = 1.3 mol

so, y = 1.3 mol

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â SO2(g) + NO2(g) ----> SO3 (g) + NO (g)

At equilibrium:Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 2.73-1.3 Â Â Â Â Â Â x-1.3 Â Â Â Â Â Â Â Â Â Â 1.3 Â Â Â Â Â Â Â Â Â Â Â Â Â 1.3

At equilibrium:Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 1.43 Â Â Â Â Â Â x-1.3 Â Â Â Â Â Â Â Â Â Â 1.3 Â Â Â Â Â Â Â Â Â Â Â Â Â 1.3

Kc= [SO3][NO] /{[SO2][NO2]}

2.9 = 1.3*1.3 / (1.43 *(x-1.3))

x-1.3 = 0.41

x = 1.71 mol

Answer: Number of moles of NO2 added = 1.71 mol

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