In an analysis of the following reaction at a certain temperature, Br2(g) + Cl2(g) ⇌ 2BrCl(g)the equilibrium concentrations were found to be [Br2] = 4.5 ×10−3 M, [Cl2] = 2.6 ×10−2 M, and [BrCl] = 1.6 ×10−2 M. Write the equilibrium expression, and calculate the equilibrium constant for this reaction at this temperature.

The equilibrium expression is Equilibrium constant =  

Kc or equilibrium constant for this reaction is 0. 55 x

Explanation:

Br2(g) + Cl2(g) ⇌ 2BrCl(g)

Equilibrium constant =  

Kc =   equation 1

      the concentration of diatoms will be divided by 2

1.3 x 10^-2 is concentration of chlorine

0.45 x 10^-2 is concentration of bromine

1.6 ×10−2 is concentration of BrCl2

Putting the values in equation 1 to calculate equilibrium constant.

Kc=    

Kc =  

Kc= 0.55 x 10^2

equilibrium constant for this reaction is 0.55 x

the molar concentration or partial pressure of the gases is taken to find the equilibrium constant.

each  column  of the  table  is called a group. elements in a group share similar properties. groups are  read  from  top  to  bottom. metal. metalloid. nonmetal. solid. liquid. gas. fe. hg. o.  2. 3. 4. 5. 6. 7. 8. 9.  2. beryllium. 9.012. 4.  sodium. 22.990.  11. 3.  magnesium. 24.305.  12.  potassium. 39.098.  19. 4.  calcium. 40.078.  20. i guess  i