The equilibrium constant, kc, for the following reaction is 1.29×10-2 at 600 k. cocl2(g) co(g) + cl2(g) calculate the equilibrium concentrations of reactant and products when 0.323 moles of cocl2(g) are introduced into a 1.00 l vessel at 600 k.

Answer : The equilibrium concentrations of are, 0.2646, 0.0584 and 0.0584.

Explanation : Given,

Moles of   = 0.323 mole

Volume of solution = 1 L

Initial concentration of = 0.323 M

Let the moles of be, 'x'. So,

Concentration of = x M

Concentration of = x M

The given balanced equilibrium reaction is,

Initial conc.          0.323 M          0          0

At eqm. conc.    (0.323-x) M    (x M)       (x M)

The expression for equilibrium constant for this reaction will be,

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

By solving the term 'x', we get :

x = 0.0584

Thus, the concentrations of at equilibrium are :

Concentration of = (0.323-x) M  = (0.323-0.0584) M = 0.2646 M

Concentration of = x M = 0.0584 M

Concentration of = x M = 0.0584 M

Therefore, the equilibrium concentrations of are, 0.2646, 0.0584 and 0.0584.

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.  

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