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Ch. 9 Stoichiometry
Terms:
Molar Mass - the mass of one mole of a chemical element or chemical compound.
Molar Ratio - conversion factors
Limiting Reactant - The reactant in a chemical reaction that limits the amount of product that can be formed.
Excess Reactant - The reactant in a chemical reaction that remains when a reaction stops when the limiting reactant is completely consumed.
Percent Yield - The actual yield of an experiment divided by the theoretical yield and multiplied by 100.
Ch. 10: Physical Characteristics of Gases
Terms:
Ideal gas - all collisions between atoms or molecules are perfectly elastic and there are no intermolecular attractive forces.(PV=NRT)
Elastic Collision - a collision in which the total kinetic energy of the colliding bodies after collision is equal to their total kinetic energy before collision.
Fluid - Anything that flows, either liquid or gas. Some solids can also exhibit fluid behavior over time.
Diffusion - The movement of a substance from an area of high concentration to an area of low concentration.
Effusion - The process by which a gas escapes through a pinhole into a vacuum.
Pressure - The force exerted by the interaction of the atmosphere and gravity. Also known as atmospheric pressure.
Barometer - An instrument, often using a column of mercury, for measuring atmospheric pressure.
Boyles Law - The pressure of a gas increases as the amount of space it is squeezed into becomes smaller.
Charles's Law - The volume of a gas at constant pressure is directly proportional to the temperature. In other words, if you heat something up, it gets big.
Gay-Lussac's Law - at a constant volume, the pressure of a confined ideal gas is proportional to temperature. In essence, as the temperature increases, the pressure will also increase.
Combined Gas Law - the combination of Boyle's, Charles's, and Gay-Lussac's Laws.
Dalton's Law of Partial Pressures - the pressure exerted by a mixture of gases equals the sum of the partial pressures of the gases in the mixture; the pressure of a gas in a mixture equals the pressure it would exert if it occupied the same volume alone at the same temperature.
Absolute Zero - The lowest possible temperature in the universe, at which all atomic activity ceases. Equal to -273 degrees Celsius (- 459 degrees Fahrenheit).
ch. 11: Molecular Composition of Gases
Terms:
Molar Volume - Molar volume is equal to the atomic weight divided by the density.
Avagadro's Law - equal volumes of all gases (given the same temperature and pressure) contain equal numbers of molecules
Ideal Gas Law - A relation among the four thermodynamic variables [Volume (V), absolute temperature (T), pressure (P), and mass, given in moles (n)] that govern the behavior of an ideal gas. This relation has the following form: PV = nRT in which R is the universal gas constant.
Ideal Gas Constant - The gas constant (also known as the universal or ideal gas constant, usually denoted by symbol R) is a physical constant used in equations of state to relate various groups of state functions to one another.
Ch. 12: Liquids and Solids
Terms:
Surface Tension - the attraction of molecules to each other on a liquid's surface. Thus, a barrier is created between the air and the liquid.
Surfactant - Any substance that when dissolved in an aqueous solution reduces its surface tension between it and another liquid.
Capillary action/rise - a force that causes liquids to rise or fall when inside very small tubular spaces.
Vaporization - The change of a substance from a liquid or solid state to the gaseous state.
Evaporation - The physical change of state of a substance from a liquid to a gas or vapor
Crystal - A crystal is a solid in which the constituent atoms, molecules, or ions are packed in a regularly ordered, repeating pattern extending in all three spatial dimensions.
Amorphous - A metal lacking distinct crystalline structure with random arrangement of atoms or molecules.
Crystal Structure - the arrangement of atoms when the element is in its solid state
Unit Cell - The smallest part of a crystal lattice structure which has all the elements of the structure of that lattice.
Equilibrium - a state of balance between opposing forces or elements.
Le Chatelier's principle - when a system at equilibrium is subjected to a stress, the equilibrium will shift in the direction that tends to counteract or relieve the effect of the stress.
Equilibrium vapor pressure - The pressure of a vapor in equilibrium with its condensed phase (liquid or solid). This equilibrium is dynamic in that evaporation and condensation are both occurring but are in equilibrium.
Volatile - Any substance that evaporates readily.
Molar heat of vaporization/fusion - tells you how much energy is needed to melt each mole of substance on hand. (Or, if you are cooling off a substance, how much energy per mole to remove from a substance as it solidifies.
Sublimation - The transition of a substance from the solid phase directly to the vapor phase, or vice versa, without passing through an intermediate liquid phase.
Terms:
Molar Mass - the mass of one mole of a chemical element or chemical compound.
Molar Ratio - conversion factors
Limiting Reactant - The reactant in a chemical reaction that limits the amount of product that can be formed.
Excess Reactant - The reactant in a chemical reaction that remains when a reaction stops when the limiting reactant is completely consumed.
Percent Yield - The actual yield of an experiment divided by the theoretical yield and multiplied by 100.
Ch. 10: Physical Characteristics of Gases
Terms:
Ideal gas - all collisions between atoms or molecules are perfectly elastic and there are no intermolecular attractive forces.(PV=NRT)
Elastic Collision - a collision in which the total kinetic energy of the colliding bodies after collision is equal to their total kinetic energy before collision.
Fluid - Anything that flows, either liquid or gas. Some solids can also exhibit fluid behavior over time.
Diffusion - The movement of a substance from an area of high concentration to an area of low concentration.
Effusion - The process by which a gas escapes through a pinhole into a vacuum.
Pressure - The force exerted by the interaction of the atmosphere and gravity. Also known as atmospheric pressure.
Barometer - An instrument, often using a column of mercury, for measuring atmospheric pressure.
Boyles Law - The pressure of a gas increases as the amount of space it is squeezed into becomes smaller.
Charles's Law - The volume of a gas at constant pressure is directly proportional to the temperature. In other words, if you heat something up, it gets big.
Gay-Lussac's Law - at a constant volume, the pressure of a confined ideal gas is proportional to temperature. In essence, as the temperature increases, the pressure will also increase.
Combined Gas Law - the combination of Boyle's, Charles's, and Gay-Lussac's Laws.
Dalton's Law of Partial Pressures - the pressure exerted by a mixture of gases equals the sum of the partial pressures of the gases in the mixture; the pressure of a gas in a mixture equals the pressure it would exert if it occupied the same volume alone at the same temperature.
Absolute Zero - The lowest possible temperature in the universe, at which all atomic activity ceases. Equal to -273 degrees Celsius (- 459 degrees Fahrenheit).
ch. 11: Molecular Composition of Gases
Terms:
Molar Volume - Molar volume is equal to the atomic weight divided by the density.
Avagadro's Law - equal volumes of all gases (given the same temperature and pressure) contain equal numbers of molecules
Ideal Gas Law - A relation among the four thermodynamic variables [Volume (V), absolute temperature (T), pressure (P), and mass, given in moles (n)] that govern the behavior of an ideal gas. This relation has the following form: PV = nRT in which R is the universal gas constant.
Ideal Gas Constant - The gas constant (also known as the universal or ideal gas constant, usually denoted by symbol R) is a physical constant used in equations of state to relate various groups of state functions to one another.
Ch. 12: Liquids and Solids
Terms:
Surface Tension - the attraction of molecules to each other on a liquid's surface. Thus, a barrier is created between the air and the liquid.
Surfactant - Any substance that when dissolved in an aqueous solution reduces its surface tension between it and another liquid.
Capillary action/rise - a force that causes liquids to rise or fall when inside very small tubular spaces.
Vaporization - The change of a substance from a liquid or solid state to the gaseous state.
Evaporation - The physical change of state of a substance from a liquid to a gas or vapor
Crystal - A crystal is a solid in which the constituent atoms, molecules, or ions are packed in a regularly ordered, repeating pattern extending in all three spatial dimensions.
Amorphous - A metal lacking distinct crystalline structure with random arrangement of atoms or molecules.
Crystal Structure - the arrangement of atoms when the element is in its solid state
Unit Cell - The smallest part of a crystal lattice structure which has all the elements of the structure of that lattice.
Equilibrium - a state of balance between opposing forces or elements.
Le Chatelier's principle - when a system at equilibrium is subjected to a stress, the equilibrium will shift in the direction that tends to counteract or relieve the effect of the stress.
Equilibrium vapor pressure - The pressure of a vapor in equilibrium with its condensed phase (liquid or solid). This equilibrium is dynamic in that evaporation and condensation are both occurring but are in equilibrium.
Volatile - Any substance that evaporates readily.
Molar heat of vaporization/fusion - tells you how much energy is needed to melt each mole of substance on hand. (Or, if you are cooling off a substance, how much energy per mole to remove from a substance as it solidifies.
Sublimation - The transition of a substance from the solid phase directly to the vapor phase, or vice versa, without passing through an intermediate liquid phase.