To determine how the reaction will shift when hydrogen gas ([tex]$H_2$[/tex]) is removed, we can apply Le Chatelier's Principle. Le Chatelier's Principle states that if a system at equilibrium is disturbed by a change in concentration, pressure, or temperature, the system will shift its equilibrium position to counteract the disturbance.
Let's consider the reaction:
[tex]\[ N_{2(g)} + 3 H_{2(g)} \rightleftharpoons 2 NH_{3(g)} \][/tex]
This reaction is in equilibrium, meaning the rate of the forward reaction (forming [tex]$NH_3$[/tex]) is equal to the rate of the reverse reaction (forming [tex]$N_2$[/tex] and [tex]$H_2$[/tex]).
1. Removing [tex]$H_2$[/tex] Gas:
- Removal of [tex]$H_2$[/tex] decreases the concentration of one of the reactants.
- According to Le Chatelier's Principle, the system will attempt to counteract this change by producing more [tex]$H_2$[/tex].
- To produce more [tex]$H_2$[/tex], the equilibrium will shift towards the reverse direction (to the left).
2. Effect of the Shift:
- By shifting to the left, the system will convert some of the [tex]$NH_3$[/tex] back into [tex]$N_2$[/tex] and [tex]$H_2$[/tex].
- This process will increase the concentration of [tex]$H_2$[/tex] back towards the equilibrium concentration.
Therefore, when [tex]$H_2$[/tex] is removed, the equilibrium of the reaction shifts to the left (in the reverse direction) to make more [tex]$H_2$[/tex] and partially restore the balance.
Conclusion:
The removal of hydrogen gas ([tex]$H_2$[/tex]) will result in the equilibrium shifting to the left (in the reverse direction) to produce more [tex]$H_2$[/tex].
Thus, the correct answer is:
- Shift left (in the reverse direction) to make more reactants
