Hills Perkins
12/28/2023 · Middle School

Consider the following equilibrium system: \[ \mathrm{PCl}_{5}(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \] A 10.00 L evacuated flask is filled with \( \mathbf{0 . 4 4 1 4} \) mol \( \mathrm{PCl}_{5}(\mathrm{~g}) \) at \( \mathbf{2 9 8 . 3} \mathrm{K} \). The temperature is then raised to 503.3 K , where the decomposition of \( \mathrm{PCl}_{5} \) gas takes place to an appreciable extent. When equilibrium is established, the total pressure in the flask is \( \mathbf{2 . 5 9 7} \) atm.

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The equilibrium calculations suggest that a significant amount of \( \mathrm{PCl}_{5} \) decomposes, but the initial assumption of \( x \) was too high, leading to a negative concentration. This indicates a need to reevaluate the equilibrium constant or the initial assumptions.

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