Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas: PCl₃(g)+Cl₂(g)⇌PCl₅(g). A 7.5-L gas vessel is charged with a mixture of PCl₃(g) and Cl₂(g), which is allowed to equilibrate at 450 K. At equilibrium the partial pressures of the three gases are PPCl₃ = 0.129 atm, PCl₂ = 0.156 atm, and PPCl₅ = 1.40 atm. What is the value of Kp at this temperature? Express your answer using three significant figures.

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OlaMacgregor OlaMacgregor · Answer 1 · 2019-10-14T10:38:17+02:00

Explanation:

As the given reaction is as follows.

[tex]PCl_{3}(g) + Cl_{2}(g) \rightleftharpoons PCl_{5}(g)[/tex]

Hence, expression for [tex]K_{p}[/tex] will be as follows.

[tex]K_{p} = \frac{P_{PCl_{5}}}{P_{PCl_{3}}P_{Cl_{2}}}[/tex]

Now, putting the given values into the above formula as follows.

[tex]K_{p} = \frac{P_{PCl_{5}}}{P_{PCl_{3}}P_{Cl_{2}}}[/tex]

= [tex]\frac{1.40 atm}{0.129 atm \times 0.156 atm}[/tex]

= 69.6

Therefore, we can conclude that the value of [tex]K_{p}[/tex] is 69.6.