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.
<u>Answer:</u> The final concentration of is 0.0012 M
<u>Explanation:</u>
We are given:
Initial concentration of = 0.0067 M
For the given chemical equation:
<u>Initial:</u> 0.0067
<u>At eqllm:</u> 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