Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl5(g) ⇌ PCl3(g) + Cl2(g) At 250° 13.0 g of PCl5 is added to the flask with a final solution volume of 0.500 L. If the value of Kc at this temperature is 1.80, what are the equilibrium concentrations of each gas?

Explanation:

Hello,

In this case, for the given chemical reaction at equilibrium, we can write the law of mass action as shown below:

That in terms of the ICE methodology is written by means of the change due to the reaction extent:

Thus, we need to compute the initial concentration of phosphorous pentachloride:

So we write:

That we solve via either solver or quadratic equation to obtain the solution:

Thereby, the equilibrium concentrations are:

Best regards.

increased stability in the completion of fluorine's outer shell.

the correct answer would be b. amelia, because the particals of gas move really fast (charged particals) and gas also has a lot of room (particals move independently) so the only answer that has both of those is amelia's.