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

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Chemistry

Phosphorus pentachloride decomposes at higher temperatures.

PCl5(g) ⇄ PCl3(g) + Cl2(g)

An equilibrium mixture at some temperature consists of

3.03 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 beaffected and what will the concentration of PCl5 be whenequilibrium is reestablished?

shift left

shift right

no shift will occur

[PCl5] =   mol/L

Answer & Explanation Solved by verified expert
4.3 Ratings (922 Votes)
Were given the following equilibriumPCl5g PCl3g Cl2gFirst we are asked to determine the    See Answer
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