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

gold is my favorite solid.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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