Chemical Equilibrium and Gas Laws Quiz

Summary Title: The Principles of Chemical Equilibrium and Gas Laws

• Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate.
• Equilibrium is reached when there is no net change in the concentration of reactants and products.
• Homogeneous equilibrium occurs when the products and reactants of an equilibrium reaction form a single phase.
• Heterogeneous equilibrium occurs when the reactant, products, or both are in more than one phase.
• KC and KP are ways to define equilibrium and are based on molar concentrations and partial pressures of gasses, respectively.
• Kinetic molecular theory explains that matter is made of tiny particles called molecules that are in constant random motion and possess kinetic and potential energy.
• Pressure is the force exerted by gas molecules colliding with the walls of a container and depends on the number of impacts per unit time and the force of each impact.
• Atmospheric pressure is the pressure exerted on us by the weight of gases in the atmosphere and decreases with height.
• Temperature is the measure of the average kinetic energy of the particles in a gas, and the hotter the temperature of gas is, the faster its molecules move.
• Boyle's law states that for a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure.
• Charles's law states that the volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant.
• Gay-Lussac's law states that the pressure of a gas is directly proportional to the Kelvin temperature if the volume remains constant.
• The combined gas law describes the relationship among pressure, volume, and temperature when only the amount of gas is constant.