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Phosphorous pentachloride decomposes at higher temperatures. PCl5(g) ⇌ PCl3(g) + Cl2(g) An equilibrium mixture at some temperature consists of 3.45 g PCl5, 208.23 g/mol 4.86 g PCl3, 137.33 g/mol 3.59 g Cl2, 70.91 g/mol in a 1.00 L-flask. If you add 1.31 g of Cl2, how will the equilibrium be affected and what will the concentration of PCl5 be when equilibrium is reestablished? a) shift left b) shift right c) no shift will occur