Iodine and bromine react to give iodine monobromide, IBr. Ilg) + Br2(g) 2 Br(g) What is the equilibrium composition of a mixture at 145 C that initially contained 0.0019 mol each of iodine and bromine in a 5.0-L vessel? The equilibrium constant K, for this reaction at 145 C is 108.

Equilibrium concentration of = 0.00006 M

equilibrium concentration of = 0.00006 M

and equilibrium concentration of  = 0.00064 M

Explanation:

Initial moles of   = 0.0019 mole

Volume of container = 5.0 L

Initial concentration of  

initial concentration of

The chemical reaction for the decomposition of phosgene follows the equation:

Initial conc.        0.00038 M       0.00038 M       0

At eqm. conc.    ( 0.00038-x) M   (0.00038-x) M  (2x) M

The expression for equilibrium constant for this reaction will be,

Thus equilibrium concentration of  = (0.00038-x) M =(0.00038-0.00032) M = 0.00006 M

equilibrium concentration of = (0.00038-x) M =(0.00038-0.00032) M = 0.00006 M

equilibrium concentration of = 2x M = 2(0.00032) M=0.00064 M

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

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