Question

At a particular temperature a 2.00-L flask at equilibrium contains 2.10E-4 mole of N2, 2.50E-5mole of O2, and 2.00E-2 mole of N2O . Calculate K at this temperature for the reaction

2N2(g)+O2(g)= 2N2O(g)

K = ___________

If [N2] = 2.00E-4 M, [N2O] = 0.200 M, and [O2] = 0.00138 M, does this represent a system at equilibrium?

_____(Yes or No)

Answer 1

Equilibrium constant K=[N₂O]² /[N₂]² [O₂] = [2.00E-2] / [2.10E-4][2.50E-5]

K=1.45X10¹³

If the stress applied to a system in equilibrium is a change in the concentration of a component of the equilibrium, the system shifts to counteract that change. If the concentration of a substance is increased, the reaction that consumes that substance is favored, and the equilibrium shifts away from that substance. If the concentration of a substance is decreased, the reaction that produces that substance is favored, and the equilibrium shifts toward that substance.

And therefore the second case where oxygen concentration is reduced ([O₂]=0.00138 M), it will be no longer in equilibrium.