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

Question

At a certain temperature, the equilibirum constant for the following chemical equation is 2.90.

SO2(g) + NO2(g) <> SO3(g) + NO(g)

At this temperature, calculate the number of moles of NO2(g) that must be added to 2.99 mol of SO2(g) in order to form 1.30 mol of SO3(g) at equilibirum. I cant get this one right please help

At a certain temperature, the equilibrium constant for the following chemical equation is 2.90 solg) + NO2(g) S03(g) + NO(g) At this temperature, calculate the number of moles of NO2(g) that must be added to 2.99 mol of SO2(g) in order to form 1.30 mol of SO3(g) at equilibrium. Number 1.16 mol of NO,u)

Explanation / Answer

K = 2.9

NO2 needed for

Before Eq

SO2 = 2.99

NO2 = y

SO3 = 0

NO = 0

In equilibrium

SO2 = 2.99 - x

NO2 = y -x

SO3 = 0 + x = 1.3

x = 1.3

NO = 0+x = 1.3

then

SO2 = 2.99 - x = 2.99-1.3 = 3.887 EROR! actual value --> 1.69

NO2 = y -x = y - 1.3

Substitut ein K

K = [SO3][NO]/[SO2][NO2]

2.9 = (1.3)(1.3)/((1.69)*(y-1.3))

Solve for y

2.9(y-1.3) = 1

y-1.3 = 1/2.9 =0.3448

y = 1.3+ 0.3448 = 1.6448

mol of NO2 needed = 1.6448 mol

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