Phosphorus pentachloride decomposes at high temperatures. PCI_5(g) PCI_3(g) + CI

Question

Phosphorus pentachloride decomposes at high temperatures. PCI_5(g) PCI_3(g) + CI_2(g) An equilibrium mixture at some temperature consists of 4.60 g PCI_5 4.86 g PCI_3 3.59 g CI_2 in a 1.00-L flask. If you add 1.31 g of CI_2, how will the equilibrium be affected? shift left shift right no shift will occur What will the concentration of PCI_5 be when equilibrium is rcestablished after addition of 1.31 g CI_2? PCI_5(g) PCI_3(g) + CI_2(g) Original Equilibrium Mixture: 4.60 g PCI_5 4.86 g PCI_3 3.59 g CI_2 in a 1.00-L flask. [PCI_5] = mol/L

Explanation / Answer

A) according to lechatlier principle concentration of products increages equilibrium shifts towards reactant side .

So equilibrium shift towards left .

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