The correct answer is option 1: decreasing the temperature.
According to Le Chatelier's principle, if the forward reaction is endothermic (requires energy), decreasing the temperature will shift the equilibrium towards the product side to compensate for the loss of energy. Therefore, decreasing the temperature will increase the amount of product at equilibrium.
Removing or adding more product will not have a significant effect on the equilibrium since the reaction is already at equilibrium.
Increasing the pressure will only affect equilibria involving gases, not liquids. Since both reactants and products are liquids in this case, increasing the pressure will not have any effect on the equilibrium.
At equilibrium, a reversible reaction contains more reactants than products. Both are liquids. The forward reaction requires energy. Which of the following adjustments will increase the amount of product at equilibrium?
1. decreasing the temperature
2. removing the product
3. adding more product
4. increasing the pressure
1 answer