The question is incomplete, here is the complete question:
Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas:
[tex]PCl_3(g)+Cl_2(g)\rightleftharpoons PCl_5(g)[/tex]
A gas vessel is charged with a mixture of [tex]PCl_3(g)[/tex] and [tex]Cl_2(g)[/tex], which is allowed to equilibriate at 450 K. At equilibrium the partial pressures of the three gases are [tex]p_{PCl_3(g)}[/tex] = 0.126 atm , [tex]p_{Cl_2(g)}[/tex] = 0.156 atm , and [tex]p_{PCl_5(g)}[/tex] = 1.60 atm. What is the value of [tex]K_p[/tex] at this temperature?
Answer: The [tex]K_p[/tex] for the given reaction is 81.4
Explanation:
For the given chemical equation:
[tex]PCl_3(g)+Cl_2(g)\rightleftharpoons PCl_5(g)[/tex]
The expression of [tex]K_p[/tex] for above reaction follows:
[tex]K_p=\frac{p_{PCl_5}}{p_{Cl_2}\times p_{PCl_3}}[/tex]
We are given:
[tex]p_{PCl_5}=1.60atm\\p_{PCl_3}=0.126atm\\p_{Cl_2}=0.156atm[/tex]
Putting values in above equation, we get:
[tex]K_p=\frac{1.60}{0.156\times 0.126}\\\\K_p=81.4[/tex]
Hence, the [tex]K_p[/tex] for the given reaction is 81.4
