Mercury and oxygen react to form mercury(ii) oxide, like this: 2hg (l) + o2 (g) → 2hgo (s) at a certain temperature, a chemist finds that a 5.2l reaction vessel containing a mixture of mercury, oxygen, and mercury(ii) oxide at equilibrium has the following composition: compound amount hg 14.7g o2 13.4g hgo 17.8g calculate kc for this reaction

Kc = 12.4 M⁻¹

Explanation:

1) Chemical equilibrium

2Hg (l) + O₂ (g) ⇄ 2HgO (s) (the double arrow indicates an equilibrium reaction)

2) Equilibrium constant, Kc:

The equilibrium constant, Kc, is equal to product of the concentrations of each product,each raised to its stoichiometric coefficient / product of the concentrations of each reactant each raised to its stoichiometric coefficient.Since the concentrations of liquid and solid substances remain practically constant, their value is incorporated into the constant Kc, and the equation only uses the concentrations of the aqueous or gaseous substances.

Thus, the equation to use is:

Kc = 1 / [O₂(g) ]

3) Determine the concentration of O₂ (g)

M = number of moles / volume in litersNumber of moles = mass in grams / molar massNumber of moles of O₂ (g) = 13.4 g / 32.00 g/mol = 0.419 mol M = 0.419 mol / 5.2 liter = 0.0806 mol / liter = 0.0806 M

4) Compute Kc

Kc = 1 / 0.0 806 M = 12.4 M⁻¹ ← answer

It’s b. mass i searched it up

What does that mean you dum bum