PCl5(g) ⇋ PCl3(g) + Cl2(g)
PCl5(g) decomposes into PCl3(g) and Cl2(g) according to the equation above. A pure sample of PCl5(g) is placed in a rigid, evacuated 1.00L container. The initial pressure of the PCl5(g) is 1.00 atm. The temperature is held constant until the PCl5(g) reaches equilibrium with its decomposition products.
If the decomposition reaction were to go to completion, the total pressure in the container will be:

A) 1.4 atm B) 2.0 atm C) 2.8 atm D) 3.0 atm

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BatteringRam BatteringRam · Answer 1 · 2020-04-28T08:05:42+02:00

Answer: The total pressure in the container is 2.00 atm

Explanation:

We are given:

Initial pressure of [tex]PCl_5[/tex] = 1.00 atm

For the given chemical equation:

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

After the completion of reaction:

Pressure of [tex]PCl_3[/tex] = 1.00 atm

Pressure of [tex]Cl_2[/tex] = 1.00 atm

Total pressure of the container = [tex]p_{PCl_3}+p_{Cl_2}=[1.00+1.00]=2.00atm[/tex]

Hence, the total pressure in the container is 2.00 atm

AFOKE88 AFOKE88 · Answer 2 · 2021-11-26T14:22:19+01:00

The total pressure in the container will be;

Option B: 2.0 atm

The given chemical reaction is;

PCl5(g) ⇋ PCl3(g) + Cl2(g)

The above chemical reaction means that;

PCl5(g) decomposes into PCl3(g) and Cl2(g).

We are given;

Initial pressure of the PCl5(g) = 1.00 atm.

Now, we are told that the temperature is held constant until the PCl5(g) reaches equilibrium with its decomposition products.

This means the decomposition products must each have a pressure of 1 atm same as the PCl5(g)

Since PCl3(g) and Cl2(g) each have a pressure of 1 atm, it means that;

Total pressure in the container = 1 + 1

Total pressure in the container = 2 atm

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