Consider the following reaction: PCl5(g) ➞ PCl3(g) +Cl2(g)a. Write the equilibrium expression for the reactionb. Initially, 0.60 mol of PCl5 is placed in a 1.0-L flask. At equilibrium, there is 0.16 mol of PCl3 in the flask. What are the equilibrium concentrations of PCl5 and Cl2?c. What is the numerical value of the equilibrium constant, Kc, for the reaction?d. If 0.20 mol of Cl2 is added to the equilibrium mixture, will the concentration of PCl5 increase or decrease?

Question
Asked Dec 1, 2019

Consider the following reaction: PCl5(g) ➞ PCl3(g) +Cl2(g)

a. Write the equilibrium expression for the reaction

b. Initially, 0.60 mol of PCl5 is placed in a 1.0-L flask. At equilibrium, there is 0.16 mol of PCl3 in the flask. What are the equilibrium concentrations of PCl5 and Cl2?

c. What is the numerical value of the equilibrium constant, Kc, for the reaction?

d. If 0.20 mol of Cl2 is added to the equilibrium mixture, will the concentration of PCl5 increase or decrease?

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Expert Answer

Step 1

Hello. Since your question has multiple sub-parts, we will solve first three sub-parts for you. If you want remaining sub-parts to be solved, then please resubmit the whole question and specify those sub-parts you want us to solve.

Step 2

The PCl molecule decomposes into the PCl3 and Cl2 gaseous molecule. The chemical reaction for this is shown in equation (1).

PCI, (g)PC, (g)+ Cl (g) )
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PCI, (g)PC, (g)+ Cl (g) )

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Step 3

The equilibrium equation for the chemical equation, shown in equation (1), is written as shown in equation (2). Where KC is the equilibrium constant, [PCl5], [PC...

[РCL|C,]
Кс
-(2)
[РC,]
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[РCL|C,] Кс -(2) [РC,]

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