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Phosphorus pentachloride decomposes at higher temperatures. PCl5(g) ⇄ PCl3(g) + Cl2(g) An equilibrium mixture at some temperature consists...

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Chemistry

Phosphorus pentachloride decomposes at highertemperatures.

PCl5(g) ⇄ PCl3(g) + Cl2(g)

An equilibrium mixture at some temperature consists of

5.93 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 affectedand what will the concentration of PCl5 be when equilibrium isreestablished?

shift left
shift right
no shift will occur
[PCl5] = mol/L

Answer & Explanation Solved by verified expert
3.6 Ratings (380 Votes)
At first equilibrium the concentrations are calculated as shownbelowThe equilibrium constant131 g of chlorine is added New    See Answer
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