It makes it difficult with no arrow. I have rewritten the equation and moved the dH so you can see it is an endothermic reaction.
2NOBr(g)+ heat =>2NO(g) + Br2(g)
Remember Le Chatelier's Principle says that when a system at equilibrium is disturbed, it will shift so as to undo what we've done to it.
a. Increased P shifts to the side with fewer mols. So decreasing P will shift to the side with more moles and that is the products.
b. Adding NO and the reaction tries to get rid of the NO added. Shifts to the left.
c. Removing Br2 means the rxn will try to add more Br2. Shift to the right.
d. Raise T and rxn tries to use up the added T. Shifts to the right.
e. Add ing NOBr and rxn tries to use it up. Shifts to the right.
For the following reaction at equilibrium, which change would shift the position of equilibrium toward forming more products? (Circle your answer(s) as there may be more than one.)
2NOBr(g) 2NO(g) + Br2(g), ∆Hºrxn = +30 kJ/mol
A) Decrease the total pressure by increasing the volume. B) Add NO. C) Remove Br2. D) Raise the temperature. E) Add NOBr
1 answer