Please help with the following physical chemistry problem.
Consider the exothermic reaction 2NO(g) + Br2(g) <----> 2NOBr(g). What can you do to the reaction mixture to produce more NOBr?
(Choose from the following choices:)
(a) Decrease T
(b) Remove Br2
(c) Add Br2
(d) Add NOBr
(e) Decrease P
(f) Remove NO
(g) Increase T
(h) Add NO
(i) Remove NOBr
(j) Increase P
Le Chatelier's principle says that a system adjusts to minimize stress. Consequently, the equilibrium shifts such that whatever is added is removed.
First take a look the concentration changes:
The concentration can be changed by adding or removing a substance. If added, the equilibrium shifts to remove the substance. If removed, the equilibrium shifts to replace it.
(b) removing Br2: because the reactant is removed, the equilibrium shifts to the left to replace it. so it does not work ...
The following posting explains how the given factors change the direction of the exothermic reaction. The solution is detailed and has a '5/5' rating.