Question

At a certain temperature, the equilibrium constant for the following chemical equation is 2.40. SO2(g)+NO2(g) -->...

At a certain temperature, the equilibrium constant for the following chemical equation is 2.40. SO2(g)+NO2(g) --> SO3 (g) + NO(g) At this temperature, calculate the number of moles of NO2(g) that must be added to 2.42 mol of SO2(g) in order to form 1.10 mol of SO3(g) at equilibrium.

Homework Answers

Answer #1

consider 1 L of solution

intially

[S02] = 2.42

let [N02] = y

at equilibrium

[S03] = 1.1

now

consider the given reaction

S02 + N02 --> S03 + N0

using ICE table

[S03]eq = x

[NO]eq = x

[S02] eq = 2.42 - x

[N02]eq = y - x

now

given

[S03]eq = 1.1

so

x = 1.1

so

[N0]eq = x = 1.1

[S02]eq = 2.42 - x = 2.42 - 1.1 = 1.32

[N02]eq = y -x = y - 1.1

now

S02 + N02 --> S03 + N0

Kc = [S03] [N0] / [S02] [N02]

2.4 = [1.1] [1.1] / [ 1.32 ] [ y - 1.1]

solving

we get

y = 1.48

so

1.48 moles of N02 must be added

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