Equilibrium

the ratio of product concentrations to reactant concentrations at equilibrium, with each concentration raised to a power equal to the number of moles of that substance in the balanced chemical equation. Commonly denoted by Kc, Kp, or Ksp

Ratio of the concentrations of the products to the concentrations of the reactants at any point during the reaction aside from equilibrium, where each reactant and product in the expression is raised to the power of its stoichiometric coefficient. Commonly denoted by Q.

reaction is at equilibrium

reaction proceeds left in favor of reactants

reaction proceeds right in favor of products

a state of equilibrium that occurs when the reactants and products of a reaction are present in more than one physical state

all the reactants and products are in the same physical state

an industrial process for producing ammonia from nitrogen and hydrogen by combining them under high pressure in the present of an iron catalyst

industrial method of preparing sulfuric acid by the catalytic oxidation of sulfur dioxide

Ì CO (g) + 2H2(g) CH3OH (g Used as starting materials for other chemicals + fuels Lower temp (227C)= favours exo reaction therefore higher yield Higher pressure (10000KPa)= favours forwards reaction as this decreases number of gaseous molecules BUT too high = too expensive catalyst= chromium

condition of continuous, random movement of particles but no overall change in concentration of materials

when stress is applied to a system at equilibrium, the system changes to relieve the stress

factor that affects equilibrium by the reaction shifting in the direction to restore the change in concentration of reactant/product

for a system at equilibrium, increasing temperature will shift the reaction to the left.

for a system at equilibrium, increasing temperature will shift the reaction to the right.

A system in which no matter is allowed to enter or leave

for a gaseous system at equilibrium, an increase in pressure will cause the system will shift to the side with less moles of gas.

increases the rates of both the forward and the reverse reactions equally