a. If the temperature is increased, the equilibrium will shift to the right. This is because the reaction is endothermic (it absorbs heat). When you add heat, the reaction shifts in the direction that absorbs the heat, in this case, to the right.

b. If the pressure is increased, the equilibrium will shift to the left. This is because there are more gas molecules on the right side of the equation (2 moles on the right vs 1 mole on the left). According to Le Chatelier's principle, the reaction will shift in the direction that reduces the pressure, in this case, to the left where there are fewer gas molecules.

c. If Cl2 is added, the equilibrium will shift to the left. According to Le Chatelier's principle, if you add more of a product, the reaction will shift in the direction that uses up that product, in this case, to the left.

d. If PCl3 is removed as it is formed, the equilibrium will shift to the right. According to Le Chatelier's principle, if you remove a product, the reaction will shift in the direction that produces more of that product, in this case, to the right.

Question

a. If the temperature is increased, the equilibrium will shift to the right. This is because the reaction is endothermic (it absorbs heat). When you add heat, the reaction shifts in the direction that absorbs the heat, in this case, to the right.

b. If the pressure is increased, the equilibrium will shift to the left. This is because there are more gas molecules on the right side of the equation (2 moles on the right vs 1 mole on the left). According to Le Chatelier's principle, the reaction will shift in the direction that reduces the pressure, in this case, to the left where there are fewer gas molecules.

c. If Cl2 is added, the equilibrium will shift to the left. According to Le Chatelier's principle, if you add more of a product, the reaction will shift in the direction that uses up that product, in this case, to the left.

d. If PCl3 is removed as it is formed, the equilibrium will shift to the right. According to Le Chatelier's principle, if you remove a product, the reaction will shift in the direction that produces more of that product, in this case, to the right.

Knowee AI · Accepted Answer

a. If the temperature is increased, the equilibrium will shift to the right. This is because the reaction is endothermic (it absorbs heat). When you add heat, the reaction shifts in the direction that absorbs the heat, in this case, to the right.

b. If the pressure is increased, the equilibrium will shift to the left. This is because there are more gas molecules on the right side of the equation (2 moles on the right vs 1 mole on the left). According to Le Chatelier's principle, the reaction will shift in the direction that reduces the pressure, in this case, to the left where there are fewer gas molecules.

c. If Cl2 is added, the equilibrium will shift to the left. According to Le Chatelier's principle, if you add more of a product, the reaction will shift in the direction that uses up that product, in this case, to the left.

d. If PCl3 is removed as it is formed, the equilibrium will shift to the right. According to Le Chatelier's principle, if you remove a product, the reaction will shift in the direction that produces more of that product, in this case, to the right.

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