chemical equilibrium

• The position of the equilibrium lies to the left when the concentration of reactants is greater than that of products.
• The position of the equilibrium lies to the right when the concentration of products is greater than that of reactants.
• A reaction mixture at equilibrium can be shifted by adding more reactant or product, but it will always return to its original state once disturbed.
• In an endothermic reaction, heat energy is absorbed by the system as the reaction proceeds from reactants to products.
• Le Chatelier's principle states that if an external factor changes during a reversible process, the system will shift in such a way as to counteract the change.
• A reversible reaction can be represented using two arrows pointing in opposite directions.
• Exothermic reactions release heat energy into their surroundings as they progress from reactants to products.
• If pressure increases on a gas-phase reaction, the equilibrium shifts towards the side with fewer moles of gas (reactants).
• If temperature decreases on an exothermic reaction, the equilibrium shifts towards the side with fewer moles of solid/liquid (products).
• Endothermic reactions require external heating to occur, while exothermic reactions generate enough internal heat to continue without further input.
• If temperature increases on an endothermic reaction, the equilibrium shifts towards the side with fewer moles of solid/liquid (products).
• When a reaction reaches equilibrium, there are no net changes in concentrations over time.
• An irreversible reaction cannot go backwards and only has one arrow pointing in one direction.
• Endothermic reactions absorb heat energy from their surroundings as they proceed from reactants to products.
• If a reaction is exothermic, increasing temperature shifts the equilibrium towards the reactants (left).
• If a reversible reaction is allowed to reach equilibrium, both forward and reverse reactions occur simultaneously.
• If a reaction is endothermic, decreasing temperature shifts the equilibrium towards the products (right).
• Decreasing the partial pressures of gases on either side of an equation will shift the equilibrium to the right.
• Decreasing the partial pressures of gases will shift the equilibrium to the left.
• Le Chatelier's Principle states that if a system at equilibrium experiences a change in its environment, it will respond so as to counteract the effect of the change.
• Increasing the pressure will increase the number of collisions between particles, leading to more successful collisions and faster rates of reaction.
• Changing the physical state of a substance has no effect on the position of equilibrium.
• Adding a catalyst does not affect the position of equilibrium but speeds up the rate of reaction.
• The concentration of reactants or products can be increased without affecting the position of equilibrium.
• Increasing the concentration of a substance favors the formation of more product.
• Adding a catalyst does not affect the position of equilibrium but increases the rate of reaction by providing an alternative pathway with lower activation energy.
• The position of equilibrium can be changed by changing the concentration or pressure of one of the substances involved in the reaction.
• The law of mass action states that the product of the concentrations of all species raised to their stoichiometric coefficients equals a constant value called Kc.