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kondaur [170]
3 years ago
13

Consider the reaction below. 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?
Chemistry
2 answers:
Dmitriy789 [7]3 years ago
6 0

Answer: The equilibrium constant for the given reaction is 0.0421.

Explanation:

PCl_5\rightleftharpoons PCl_3+Cl_2

Concentration of [PCl_5] =  0.0095 M

Concentration of [PCl_3] =  0.020 M

Concentration of [Cl_2] =  0.020 M

The expression of the equilibrium constant is given as:

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

K_c=0.0421 (An equilibrium constant is an unit less constant)

The equilibrium constant for the given reaction is 0.0421.

hram777 [196]3 years ago
3 0

Answer: 0.042

Explanation:- Equilibrium constant is the ratio of concentration of products to the concentration of reactants each term raised to their stochiometric coefficients.

PCl_5(g)\rightarrow PCl_3(g)+Cl_2(g)

K_c=\frac{[PCl_3][Cl_2]}{[PCl_5]}

Given :[PCl_5]= 0.0095 M

[PCl_3] = 0.020 M

[Cl_2] = 0.020 M

Putting the given values n the equation:

K_c=\frac{[0.020][0.020]}{[0.0095]}=0.042

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