1 Potassium chlorate decomposes to product potassium chloride and oxygen gas. 2KClO3(s) ⇔ 2KCl(s) + 3O2(g) When this reaction was run at room temperature, the following equilbrium concentrations were measured: [O2] = 0.0500 M; [KCl] = 0.00250 M; [KClO3] = 2.00 M What is the equilibrium constant for this reaction?

The equilibrium constant for this reaction is

Explanation:

Equilibrium constant is the ratio of the concentration of products to the concentration of reactants each term raised to its stochiometric coefficients.

The given balanced equilibrium reaction is,

At eqm. conc.     (2.00) M       ( 0.00250 ) M   (0.0500) M

The expression for equilibrium constant for this reaction will be,

Now put all the given values in this expression, we get :

By solving we get :

Thus the equilibrium constant for this reaction is

the answer is d. 74.02

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.