Question on Molarity and Solubility

[dorothylinn]

This is the chemical equation: C₂H₄(g)+Cl₂(g)⇌C₂H₄Cl₂(g)

If you were a chemist trying to maximize the amount of C₂H₄Cl₂ produced, which tactic(s) might you try? Assume that the reaction mixture reaches equilibrium.

Check all that apply.

removing C₂H₄Cl₂ from the reaction mixture as it forms

adding Cl₂

lowering the reaction temperature

increasing the reaction volume

I honestly have no idea how C₂H₄CL₂ can be maximized. I would think lowering the temperature, and maybe even increasing the reaction volume. Please help me understand what the question means and why or why not an option would make sense. This is not an exam question, just a homework question from Pearson Textbook.

[ChenBeier]

Read the principles of Le Chatelier.

Here you make from two reactants one product. So it means decrease Volume or increase pressure will give more product .Figure out is the reaction exothermic or endothermic. Means consume or release heat. If it consumes rise temperature, in other case decrease temperature.
Then adding more reactants and removing more product also drive it to a maximum.

[jesse99]

In my opinion, the best tactics to maximize C₂H₄Cl₂ production are removing C₂H₄Cl₂ as it forms and adding Cl₂. Retro Bowl

[bekeanloinse]

According to Le Chatelier's Principle, if C₂H₄Cl₂ is removed from the reaction mixture, the equilibrium will shift to produce more C₂H₄Cl₂ to counteract the loss. Therefore, removing C₂H₄Cl₂ will favor the forward reaction and increase the production of C₂H₄Cl₂.