Question

For the chemical equation SO 2 ( g ) + NO 2 ( g ) − ⇀ ↽ − SO 3 ( g ) + NO ( g ) the equilibrium constant at a certain temperature is 3.10 . At this temperature, calculate the number of moles of NO 2 ( g ) that must be added to 2.30 mol SO 2 ( g ) in order to form 1.00 mol SO 3 ( g ) at equilibrium.

Answer 1

Moles of NO₂ = 0.158

Step-by-step explanation:

SO 2 ( g ) + NO 2 ( g ) ⇄ SO 3 ( g ) + NO ( g )

According to the law of mass equation

`K_(c)` =
`([SO_(3) ][NO])/([SO_(2)][NO_(2) ])`

⇒ 3.10 =
`((1.00)(1.00))/((2.30) [NO_(2) ])` At equilibrium [SO₃] = [NO]

⇒ [NO₂] =
`(1)/(6.3)`

⇒ [NO₂] = 0.158

So. number of moles of NO₂ at equilibrium added = 0.158