A small amount of product is added to the equilibrium system below.
H2(g) + I2(g) ⇔ 2HI(g)
Predict the result.
a) The equilibrium shifts forward
b) The equilibrium shifts backward
c) There is no effect on the equilibrium
d) The change in equilibrium can not be predicted.
e) The reverse reaction no longer occurs.
a) The equilibrium shifts forward
are you sure?
I apologize for the confusion. If a small amount of product is added to an equilibrium system, the equilibrium will shift backward in order to reduce the concentration of the product and reach a new equilibrium. Therefore, the correct answer is b) The equilibrium shifts backward.
To predict the result, we need to apply Le Chatelier's principle, which states that when a system at equilibrium is subjected to a change, it will try to counteract that change and establish a new equilibrium.
In this case, a small amount of product is added to the equilibrium system. Adding product means increasing the concentration of HI (hydrogen iodide) gas.
According to Le Chatelier's principle, when the concentration of a reactant or a product is increased, the system will shift in the direction that consumes or reduces that substance.
Therefore, in this case, by adding more HI, the system will try to consume or reduce HI to establish a new equilibrium. The system will shift backward (to the left) to decrease the concentration of HI.
So, the answer is:
b) The equilibrium shifts backward.