Question

At a certain temperature, the equilibrium constant for the following chemical equation is 2.60. At this...

At a certain temperature, the equilibrium constant for the following chemical equation is 2.60. At this temperature, 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.

Homework Answers

Answer #1

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

2.64              x                                    0             0 ----------------------> initial

-y                  - y                                 +y           +y --------------------> dissociation

2.64 - y       x - y                                  y           y-----------------------> equilibrium

2.64 - 1.10      x-1.10                           1.10          1.10

1.54               x-1.10                              1.10       1.10(afetr below calculation)

at equilibrium SO3 moles given so

y = 1.10

Kc = 2.60

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

2.60 = (1.10 )^2 / (1.54) (x - 1.10)

x = 1.40

NO2 moles = x = 1.40

1.40 moles of NO2 must be added.

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