0.05mol

of

H_(2)

and

0.05mol

of

Br_(2)

are placed in an evacuated

5.0L

flask and heated to

700K

. What is the concentration of each species in the flask when equilibrium has been established? The equation for the reaction is as follows:\

H_(2)(g)+Br_(2)(g)2HBr(g),K_(c)=64@700K\ [H_(2)]=\ [Br_(2)]=\ [HBr]=,M

0.05mol of H2 and 0.05mol of Br2 are placed in an evacuated 5.0L flask and heated to 700K. What is the concentration of each species in the flask when equilibrium has been established? The equation for the reaction is as follows: H2(g)+Br2(g)2HBr(g)[H2]=[Br2]=[HBr]=Kc=64@700KMM