Two moles of PCl₅ are placed in a 5.0 L container.Dissociation takes place according to the equation PCl₅(g)
PCl₃(g)+ Cl₂(g).At equilibrium, 0.40 mol of Cl₂ are present.Calculate the equilibrium constant (K_c)for this reaction under the conditions of this experiment.

Question

Two moles of PCl₅ are placed in a 5.0 L container.Dissociation takes place according to the equation PCl₅(g) Two moles of PCl5 are placed in a 5.0 L container.Dissociation takes place according to the equation PCl5(g) PCl3(g)+ Cl2(g).At equilibrium, 0.40 mol of Cl2 are present.Calculate the equilibrium constant (Kc)for this reaction under the conditions of this experiment.

Two moles of PCl<sub>5</sub> are placed in a 5.0 L container.Dissociation takes place according to the equation PCl<sub>5</sub>(g) <sub> </sub> PCl<sub>3</sub>(g)+ Cl<sub>2</sub>(g).At equilibrium, 0.40 mol of Cl<sub>2</sub> are present.Calculate the equilibrium constant (K<sub>c</sub>)for this reaction under the conditions of this experiment.

PCl₃(g)+ Cl₂(g).At equilibrium, 0.40 mol of Cl₂ are present.Calculate the equilibrium constant (K_c)for this reaction under the conditions of this experiment.

Quizplus · Accepted Answer

The Answer of Two moles of PCl₅ are placed in a 5.0 L container.Dissociation takes place according to the equation PCl₅(g) PCl₃(g)+ Cl₂(g).At equilibrium, 0.40 mol of Cl₂ are present.Calculate the equilibrium constant (K_c)for this reaction under the conditions of this experiment.

Two Moles of PCl5 Are Placed in a 5

Two Moles of PCl₅ Are Placed in a 5