Calculate the equilibrium constant for the following reaction: 2cl2(g) + 2h2o(g) ⇌ 4hcl(g) + o2(g) given: 2mgcl2(s) + o2(g) ⇌ 2mgo(s) + 2cl2(g) k = 8.59 mgcl2(s) + h2o(g) ⇌ mgo(s) + 2hcl(g) k = 8.29

Answer : The equilibrium constant for the final reaction will be, 8.00

Explanation :

The following equilibrium reactions are :

(1)      

(2)      

The final equilibrium reaction is :

Now we have to calculate the value of for the final reaction.

First reverse the equation 1 that means we are writing the equilibrium constant as and multiplying the equation 2 by 2 that means we are writing the equilibrium constant as , we get the final equilibrium reaction and the expression of final equilibrium constant is:

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

Therefore, the equilibrium constant for the final reaction will be, 8.00

the seeing the electronic configuration we can say that the element is fluorine.

fluorine is the most electronegative element in the periodic table.

but by only seeing the configuration we cannot say about its reactivity because we don't know if its configuration after excitation or by addition of electrons.

but if not then, it is the lightest halogen and exists as a highly toxic pale yellow diatomic gas at standard conditions. as the most electronegative element, it is extremely reactive: almost all other elements, including some noble gases, form compounds with fluorine.

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