Martinez Schwartz
04/17/2024 · High 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 0.4150 mol \( \mathrm{PCl}_{5}(\mathrm{~g}) \) at 297.4 K . The temperature is then raised to 501.7 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 \( \mathbf{2 . 4 3 3} \) atm.
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At equilibrium, the amounts of each species are: \( \mathrm{PCl}_{5} \): \( 0.2400 \, \text{mol} \), \( \mathrm{PCl}_{3} \): \( 0.175 \, \text{mol} \), \( \mathrm{Cl}_{2} \): \( 0.175 \, \text{mol} \), and the total pressure in the flask is \( 2.433 \, \text{atm} \).
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