For the decomposition of phosphorous pentachloride to phosphorous trichloride and chlorine at 400K the KC is 1.1x10-2. Given that 1.0g of phosphorous pentachloride is added to a 250mL reaction flask, find the percent decomposition after the system has reached equilibrium. PCl_5(g) PCl_3(g) Cl_2(g) K_C

Explanation:

Hello,

In this case, for the given decomposition of phosphorous pentachloride:

As the equilibrium constant is and the initial concentration of phosphorous pentachloride is:

Hence, by writing the law of mass action equation:

We must introduce the change occurring due to the reaction extent and the concentrations at equilibrium (ICE table methodology):

Thus, solving for we obtain:

In such a way, the equilibrium concentration of phosphorous pentachloride results:

Finally, the percent decomposition is computed by:

Best regards.

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because it does not have the potential to be entirely used up