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.

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