Answer:
The reaction is not at equilibrium and reaction must run in forward direction.
Explanation:
At the given interval, concentration of NO = [tex]\frac{4.64\times 10^{-2}}{1}M=4.64\times 10^{-2}M[/tex]
Concentration of [tex]Br_{2}[/tex] = [tex]\frac{4.56\times 10^{-2}}{1}M=4.56\times 10^{-2}M[/tex]
Concentration of NOBr = [tex]\frac{0.102}{1}M=0.102M[/tex]
Reaction quotient,[tex]Q_{c}[/tex] , for this reaction = [tex]\frac{[NOBr]^{2}}{[NO]^{2}[Br_{2}]}[/tex]
species inside third bracket represents concentrations at the given interval.
So, [tex]Q_{c}=\frac{(0.102)^{2}}{(4.64\times 10^{-2})^{2}\times (4.56\times 10^{-2})}=106[/tex]
So, the reaction is not at equilibrium.
As [tex]Q_{c}< K_{c}[/tex] therefore reaction must run in forward direction to increase [tex]Q_{c}[/tex] and make it equal to [tex]K_{c}[/tex].
