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cricket20 [7]
3 years ago
11

The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCl3(g) Cl2(g) PCl5(g) Calculate the equilibrium conc

entrations of reactant and products when 0.453 moles of PCl3 and 0.453 moles of Cl2 are introduced into a 1.00 L vessel at 500 K.
Chemistry
1 answer:
Alik [6]3 years ago
6 0

Answer:

[PCl_3]=[Cl_2]=0.068M

[PCl_5]=0.385M

Explanation:

Hello!

In this case, since the equilibrium expression for the considered equation is:

Kc=\frac{[PCl_5]}{[Cl_2][PCl_3]}

Which can be written in terms of the reaction extent and the ICE chart and the initial concentrations of 0.453 M as shown below:

83.3=\frac{x}{(0.453M-x)(0.453M-x)}

We can solve for x as follows:

x=0.385M

In such a way, we obtain the following concentrations at equilibrium:

[PCl_3]=[Cl_2]=0.453M-0.385M=0.068M

[PCl_5]=0.385M

Best regards!

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The number of hybrid orbitals is equal to the number of atomic orbitals that are blended together. True

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