Consider the reaction below. 0.0067 M SbCl5 is placed in a one liter flask and the system is allowed to reach equilibrium. What is final concentration of SbCl5? Kc at this temperature is 2.5 x 10-2.

The question is incomplete, here is the complete question:

Consider the reaction below.

0.0067 M SbCl₅ is placed in a one liter flask and the system is allowed to reach equilibrium. What is final concentration of SbCl₅? Kc at this temperature is 2.5 x 10-2.

The final concentration of is 0.0012 M

Explanation:

We are given:

Initial concentration of = 0.0067 M

For the given chemical equation:

Initial:              0.0067

At eqllm:       0.0067-x           x              x

The expression of for above equation follows:

We are given:

Putting values in above expression, we get:

Neglecting the negative value of 'x' because concentration cannot be negative

So, final concentration of

Hence, the final concentration of is 0.0012 M

you gotta add the following molecules so we can give u an answer

explanation: