Part a what is the numerical value of kc for the following reaction if the equilibrium mixture contains 0.51 m c3h6o, 0.30 m o2, 1.8 m co2, and 2.0 m h2o? c3h6o(g)+4o2(g)⇌3co2(g)+3h2o(g)
a) 2.4 × 101b) 1.1 × 104c) 8.9 × 10-5d) 4.3 × 10-2

Explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as .

The given balanced equilibrium reaction is,

 At eqm. conc.    (0.51) M   (0.30) M   (1.8) M    (2.0)M

The expression for equilibrium constant for this reaction will be,

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

Thus the value of the equilibrium constant is

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.