At high temperature, 2.00 mol of HBr was placed in a 4.00 L container where it decomposed in the reaction: 2HBr(g) H2(g) Br2(g) At equilibrium the concentration of Br2 was measured to be 0.0955 M. What is Kc for this reaction at this temperature

for this reaction at this temperature is 0.029

Explanation:

Moles of   = 2.00 mole

Volume of solution = 4.00 L

Initial concentration of

The given balanced equilibrium reaction is,

Initial conc.              0.500 M              0  M        0 M  

At eqm. conc.            (0.500-2x) M   (x) M   (x) M

The expression for equilibrium constant for this reaction will be,

Equilibrium concentration of = x =  0.0955 M

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

Thus for this reaction at this temperature is 0.029

oxygen, selenium, tellurium, and polonium.

they're all from the same group as sulfur (group 16).