Le Chatelier's Principle and Concentration Changes

How does a decrease in temperature affect an exothermic reaction?

In gaseous reactions, what happens if there is an increase in pressure?

For a reaction that produces more moles of gas, what happens if the pressure is increased?

What happens to the yield of an endothermic reaction if the temperature is decreased?

When pressure decreases in a gaseous reaction, where does the equilibrium shift?

If a reaction produces fewer moles of gas, what happens when pressure is increased?

In which direction does the equilibrium shift if a reaction produces more moles of gas and pressure is increased?

In a closed system, when does equilibrium occur for a reversible reaction?

What happens when a reversible reaction reaches equilibrium in a closed system?

How do changing conditions affect the relative amounts of reacting substances at equilibrium?

If a reversible reaction is exothermic, what happens at equilibrium if the temperature is increased?

What is the impact on equilibrium when a reversible reaction takes place in an open system?

What happens to the position of equilibrium when the concentration of reactants is increased?

How does increasing the concentration of products affect the position of equilibrium?

If a reaction is endothermic and the temperature is increased, what is the effect on equilibrium?

In Le Chatelier's principle, what does the system do when a change is made to any of the conditions of equilibrium?

For an exothermic reaction, what happens if the temperature is decreased?

When a system is no longer at equilibrium due to a change in concentration, what occurs until equilibrium is reached again?

In a gaseous reaction that produces the least number of molecules, what happens to the equilibrium if the pressure is increased?

For a reaction producing a larger volume of gas (more moles), what happens if the pressure is decreased?

How does a decrease in temperature affect the yield of an endothermic reaction?

When a decrease in pressure occurs in a gaseous reaction, where does the equilibrium shift?

If a reaction produces fewer moles of gas, what happens when the pressure is increased?

What is the effect of pressure changes on equilibrium in gaseous reactions?

What symbol is typically used to represent a reversible reaction?

How can the direction of a reversible reaction be altered?

In which type of reactions can the products react to form the original reactants?

If a reversible reaction is endothermic in one direction, what is it in the opposite direction?

What type of change occurs if a reversible reaction is endothermic one way?

What is the relationship between an endothermic reaction and an exothermic reaction in a reversible reaction?