a mixture of 000423 mol H2 and 000414 mole Br2 was placed in

a mixture of 0.00423 mol H2 and 0.00414 mole Br2 was placed in a 3.00 L stainles steel flask at 430 degrees C. Calculate the concentration of each compound at equilibrium. The Kc is 58.3.

Solution

let the number of moles of Br dissociated be x.so

moles of Br2=0.00414-x

moles of H2=0.00423-x

moles of HBr=2x

H2+Br2--->2HBr

so,

Kc=[HBr]^2/[H2][Br2]

or 58.3=(2x)^2/((0.00414-x)(0.00423-x))

or x=0.003315

so [HBr]=2*0.003315/2

=0.003315 M

[H2]=moles/3

=0.000305 M

[Br2]=0.000275 M