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$$P{ Cl }_{ 5 }(g) \rightleftarrows P{ Cl }_{ 3 }(g) + { Cl }_{ 2 }(g)$$

Gaseous phosphorus pentachloride decomposes into phosphorus trichloride and chlorine gas, as shown by the equation above.

A pure sample of $P{ Cl }_{ 5 }(g)$ is placed into a rigid, evacuated container at a particular temperature; the initial partial pressure of $P{ Cl }_{ 5 }(g)$ is 1.00 atm, as shown in the first figure. The decomposition is allowed to occur at a constant temperature.

When reaction ceases, the system has the composition shown in the second figure, with a total pressure of 1.50 atm.

Based on the information in the figures and in the preceding description, which of the following can be concluded concerning this system?

A

The value of the equilibrium constant, ${ K }_{ p }$, is 1.00.

B

The value of the equilibrium constant, ${ K }_{ p }$, is greater than 1.00.

C

The equilibrium partial pressures of all three gases are 0.50 atm.

D

Since reaction has ceased, we can conclude that all of the $P{ Cl }_{ 5 }(g)$ has been consumed.

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