Question

At 500 K, the reaction is at equilibrium with the following concentrations. [PCI5]= 0.0095 M [PCI3] = 0.020 [CI2] = 0.020 M What is the equilibrium constant for the given reaction? 0.042 0.42 2.4 24

Answer 1

Although it is omitted, the reaction equation for the decomposition of phosphorus pentachloride is:
PCl₅ → PCl₃ + Cl₂

The equilibrium constant's equation then becomes:
Kc = [PCl₃]*[Cl₂] / [PCl₅]
Kc = (0.02 * 0.02) / 0.0095
Kc = 0.042

The equilibrium constant is 0.042.

Answer 2

Answer:The equilibrium constant for the given reaction 0.0421.

Explanation:

$PCl_5\rightaleftharpoons PCl_3+Cl_2$

$[PCl_5]=0.0095 M,[PCl_3]=0.020 M,[Cl_2]=0.020 M$

The equilibrium constant will be given by:

$K_c=\frac{[PCl_3][Cl_2]}{[PCl_5]}=\frac{0.020 M\times 0.020M}{0.0095 M}=0.0421$

The equilibrium constant for the given reaction 0.0421.