At a certain temperature, the equilibrium constant for the following chemical eq

Question

At a certain temperature, the equilibrium constant for the following chemical equation is 3.50.

SO2 + NO2 <----> SO3 + NO ( all gas)

At this temperature, calculate the number of moles of NO2(g) that must be added to 2.86 mol of SO2(g) in order to form 1.30 mol of SO3(g) at equilibrium. Please break it down step by step so i can see how to solve correctly. Thank you.

(Also,I've been having some issues with getting the right numbers on my TI 84 Plus C calculator, so if anyone knows exactly how to enter the numbers and can list those on the steps I would be extremely grateful!)

Explanation / Answer

The equilibrium constant, Keq, for the reaction = 3.50 at a certain temperature

SO2(g) +NO2(g) ? SO3(g) + NO(g)

Keq = Kc = [SO3}x[NO]/[SO2]x[NO2}

Based on given data:

[SO3] =1.3 mol = [NO]

[SO2] = 2.86 mol

So, Required amount of [NO2] =[SO3}x[NO]/[SO2]xKc = 1.3*1.3/2.86*3.50 = 2.068 mol

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