Question

Consider the following endothermic reaction: C2H4(g)+I2(g)⇌C2H4I2(g) Part A If you were a chemist trying to maximize the amount of C2H4I2 produced, which tactic(s) might you try? Assume that the reaction mixture reaches equilibrium. Check all that apply. Check all that apply. raising the reaction temperature adding more I2 to the reaction mixture adding C2H4 to the reaction mixture increasing the reaction volume

Answer 1

ANSWER:

Since, the reaction is endothermic, raising the temperature will shift the equilibrium to left side. Means reaction will move in backward direction.

Addition of I₂ to the reaction mixture will shift the equilibrium in right side means reaction will move in forward direction.

Addition of C₂H₄ to the reaction mixture will shift the equilibrium in right side means reaction will move in forward direction.

On increasing the volume of reaction vessel will decrease the molar concentration of each component which will cause the reaction to move in a direction of increasing mole. Hence, reaction will move in backward direction as moles of reactant are greater than moles of product.

So, to increase the production of C₂H₄I₂, I will use the tactics as addition of I₂ and addition of C₂H₄ to the reaction mixture.