Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction: PCl3 (g) + Cl2 (g) → PCl5 (g) An equilibrium mixture at 450 K contains PPCl3 = 0.348 atm, PCl2 = 0.441 atm, and PPCl5 = 10.24 atm. What is the value of Kp at this temperature? Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction: (g) + (g) (g) An equilibrium mixture at 450 K contains = 0.348 atm, = 0.441 atm, and = 10.24 atm. What is the value of Kp at this temperature? 66.7 1.50 ⋅ 10−2 12.99 1.57 9.45

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Alleei Alleei · Answer 1 · 2019-10-10T08:03:03+02:00

Answer : The value of [tex]K_p[/tex] at this temperature is 66.7

Explanation : Given,

Pressure of [tex]PCl_3[/tex] at equilibrium = 0.348 atm

Pressure of [tex]Cl_2[/tex] at equilibrium = 0.441 atm

Pressure of [tex]PCl_5[/tex] at equilibrium = 10.24 atm

The balanced equilibrium reaction is,

[tex]PCl_3(g)+Cl_2(g)\rightleftharpoons PCl_5(g)[/tex]

The expression of equilibrium constant [tex]K_p[/tex] for the reaction will be:

[tex]K_p=\frac{(p_{PCl_5})}{(p_{PCl_3})(p_{Cl_2})}[/tex]

Now put all the values in this expression, we get :

[tex]K_p=\frac{(10.24)}{(0.348)(0.441)}[/tex]

[tex]K_p=66.7[/tex]

Therefore, the value of [tex]K_p[/tex] at this temperature is 66.7