When the chemical reaction: Br2(g) + Cl2(g) ↔ 2 BrCl(g) is at equilibrium, which answer describes two ways that the reaction would shift to the right?
Add Cl2 and add BrCl
Add Br2 and add BrCl
Remove Br2 and add Cl2
Add Br2 and remove BrCl
Remove Br2 and add BrCl
we know that
according to Le chatlier principle
the equilibrium will shift in a direction to counter the change
so
consider the reaction
Br2 + Cl2 --> 2 BrCl
now add Br2 and Cl2
now according to Le Chatlier principle
the equilibrium will shift in a direction to remove Br2 and Cl2
so
they will be consumed and BrCl is formed
that is the equilibrium is shifted to the right
similarly
remove Br2 and Cl2
the equilibrium will shift to the left
now
remove BrCl
so
according to Le Chatlier principle
the equilibrium will shift in a direction to add BrCl
so
more and more BrCl will be formed
so
the equilibrium will shift to the right
similarly add BrCl
the equilibrium will shift to the left
now
the requirement is the equilibrium should shift to the right
to
add Br2 or Cl2 or remove BrCl
so
the answer is
Add Br2 and remove BrCl
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