Titanium(iv) chloride decomposes to form titanium and chlorine, like this: (l)(s)(g) at a certain temperature, a chemist finds that a reaction vessel containing a mixture of titanium(iv) chloride, titanium, and chlorine at equilibrium has the following composition: compound amount calculate the value of the equilibrium constant for this reaction. round your answer to significant digits.

The question is incomplete ,the complete question is:

Titanium(IV) chloride decomposes to form titanium and chlorine, like this:

At a certain temperature, a chemist finds that a 5.2 L reaction vessel containing a mixture of titanium(IV) chloride, titanium, and chlorine at equilibrium has the following composition:

Compound          amount

       4.18 g

Ti                             1.32 g

         1.08g

Calculate the value of the equilibrium constant for this reaction. Round your answer to significant digits.

the value of the equilibrium constant for this reaction.

Explanation:

We have : Volume of vessel = 5.2 L

Concentration of Titanium(IV) chloride at equilibrium =:

Concentration of Titanium at equilibrium =:

Concentration of chloride at equilibrium =:

The equilibrium expression will be given as:

The concentration of the solids and liquid is taken as unity.

the value of the equilibrium constant for this reaction.

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