Apply Le Chatelier's principle to predict whether, and in which direction, the following established equilibrium would be shifted by the change imposed:
undefined
a) temperature is decreased
b) vessel volume is decreased
c) oxygen is removed
d) platinum catalyst is added
e) carbon dioxide is added
a) When the temperature is decreased in an equilibrium system, the reaction will shift in the direction that produces heat. This is because the reaction is trying to counteract the decrease in temperature. If the reaction is exothermic, meaning it releases heat, then decreasing the temperature will shift the equilibrium towards the side of the reaction that produces more heat. If the reaction is endothermic, meaning it absorbs heat, then decreasing the temperature will shift the equilibrium towards the side of the reaction that absorbs more heat.
b) When the vessel volume is decreased in an equilibrium system, the reaction will shift in the direction that produces fewer moles of gas. This is because when the volume decreases, the pressure increases. According to Le Chatelier's principle, the equilibrium will shift in the direction that reduces the pressure. If the reaction involves a change in the number of moles of gas, then decreasing the volume will shift the equilibrium towards the side of the reaction that has fewer moles of gas.
c) When oxygen is removed from an equilibrium system, the reaction will shift in the direction that produces more oxygen. This is because removing oxygen from the system leads to a decrease in the concentration of oxygen. According to Le Chatelier's principle, the equilibrium will shift in the direction that replenishes the decreased concentration. In this case, the equilibrium will shift towards the side of the reaction that produces more oxygen.
d) When a platinum catalyst is added to an equilibrium system, it does not cause a shift in the equilibrium. A catalyst only speeds up the rate at which the equilibrium is achieved, but it does not change the position of the equilibrium. Therefore, the addition of a platinum catalyst will not result in a shift in the equilibrium in any particular direction.
e) When carbon dioxide is added to an equilibrium system, the reaction will shift in the direction that reduces the concentration of carbon dioxide. This is because adding carbon dioxide increases its concentration in the system. According to Le Chatelier's principle, the equilibrium will shift in the direction that counteracts the increase in concentration. In this case, the equilibrium will shift towards the side of the reaction that consumes more carbon dioxide.