Phosphorus pentachloride decomposes at higher temperatures. \( \mathrm{PCl}_{5}(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \) An equilibrium mixture at some temperature consists of \( 5.08 \mathrm{~g} \mathrm{PCl}_{5}, 208.23 \mathrm{~g} / \mathrm{mol} \) \( 4.86 \mathrm{~g} \mathrm{PCl}_{3}, 137.33 \mathrm{~g} / \mathrm{mol} \) \( 3.59 \mathrm{~g} \mathrm{Cl}_{2}, 70.91 \mathrm{~g} / \mathrm{mol} \) in a \( 1.00-\mathrm{L} \) flask. If you add 1.31 g of Cl reestablished? , how will the equilibrium be affected and what will the concentration of \( \mathrm{PCl}_{5} \) be when equilibrium is shifight right no shift will occur
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