At a certain temperature, the equilibrium constant for the following chemical equation is 3.30. SO2(g) + NO2(g) <---> SO3(g) + NO(g), At this temp, calculate the number of moles of NO2(g) that must be added to 2.64 mol of SO2(g) in order to form 1.10 mol of SO3(g) at equilibrium.
K = 3.3
K = SO3*NO/(SO2*NO2)
in equilibrium
[SO2] = 2.64 - x
[NO2] = y - x
[SO3] = 0 + x
[NO] = 0 +x
in equilbirium
[SO3] = 0 + x = 1.1
then
x = 1.1
[SO2] = 2.64 - 1.1 = 1.54
[NO2] = y - 1.1
[SO3] = 0 + 1.1 = 1.1
[NO] = 0 +1.1 = 1.1
solve for y
K = SO3*NO/(SO2*NO2)
3.3 = 1.1*1.1 / (1.54*(y - 1.1 ))
(y-1.1) = 1.1*1.1/(1.54*3.3)
y = 0.2380+1.1 = 1.338 mol of NO2
thats the amount we must add of NO2 in moles
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