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

Answer:

Moles of NO₂ = 0.158

Explanation:

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

              According to the law of mass equation

                                     

                                       $K_{c}$ = $\frac{[SO_{3} ][NO]}{[SO_{2}][NO_{2} ]}$

                              ⇒   3.10 = $\frac{(1.00)(1.00)}{(2.30) [NO_{2} ]}$    At equilibrium [SO₃] = [NO]

                              ⇒ [NO₂] = $\frac{1}{6.3}$

                              ⇒ [NO₂] = 0.158

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