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Vera_Pavlovna [14]

2 years ago

11

Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reactio

n: 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

1 answer:

umka21 [38]2 years ago

4 0

Answer : The value of $K_p$ at this temperature is 66.7

Explanation : Given,

Pressure of $PCl_3$ at equilibrium = 0.348 atm

Pressure of $Cl_2$ at equilibrium = 0.441 atm

Pressure of $PCl_5$ at equilibrium = 10.24 atm

The balanced equilibrium reaction is,

$PCl_3(g)+Cl_2(g)\rightleftharpoons PCl_5(g)$

The expression of equilibrium constant $K_p$ for the reaction will be:

$K_p=\frac{(p_{PCl_5})}{(p_{PCl_3})(p_{Cl_2})}$

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

$K_p=\frac{(10.24)}{(0.348)(0.441)}$

$K_p=66.7$

Therefore, the value of $K_p$ at this temperature is 66.7

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