Chapters 13 & 17 – Flashcards
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What does all matter consist of according to kinetic theory? |
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tiny particles that are constantly in motion |
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Compared to solids or liquids, gas particles are |
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relatively far apart |
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Why is the motion of one particle in a gas independent of the motion of the other particles? |
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no attractive or repulsive forces exist |
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Why do gases fill their containers regardless of shape/volume of the containers? |
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their motion is rapid, constant, and random |
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How far is a gas particle's path of uninterrupted travel? |
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very short until they collide with another particle or surface |
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What happens during an elastic collision? |
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kinetic energy is transferred without loss from one particle to another |
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Gas pressure is the result of what? |
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the force exerted by a gas per unit surface area |
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A vacuum doesn't have what two things? |
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particles and pressure |
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Why does air exert pressure on Earth? |
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gravity holds the particles within the Earth's atmosphere |
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Atmospheric pressure is the result of ... |
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collisions of atoms and molecules in air with objects |
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What does a barometer measure? |
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atmospheric pressure |
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Numerical pressure relationship between three common pressure units |
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1 atm = 760 mm Hg = 101.3 kPa |
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An increase in kinetic energy causes ... |
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an increase in temperature |
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Why is average kinetic energy used when discussing the kinetic energy of a collection of particles? |
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particles at a given temperature have a wide range of kinetic energies and most are near the average |
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There is a wider range of kinetic energies when the temperature is ... |
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increased |
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What would happen to the motion of particles if we could cool them to absolute zero? |
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motion would cease |
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Kelvin temperature of a substance is directly proportional to ... |
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the average kinetic energy of the particles of the substance |
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vaporization |
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the conversion of a liquid to a gas or vapor |
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A liquid to gas conversion at the non-boiling surface of a liquid is ... |
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evaporation |
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Why does a liquid evaporate faster when heated? |
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the average kinetic energy of the particles increases |
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Vapor pressure |
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measure of the force exerted by a gas above a liquid |
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Why does an increase in the temperature of a contained liquid increase its vapor pressure? |
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particles in the warmer liquid have increased kinetic energy |
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volatility |
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how easily a liquid evaporates |
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manometer |
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a device used to measure vapor pressure of a liquid |
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boiling point |
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the temperature at which the vapor pressure of the liquid is just equal to the external pressure on the liquid |
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Why doesn't a liquid always boil at the same temperature? |
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because a liquid boils when its vapor pressure is equal to external pressure |
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Why do boiling points decrease at high altitudes? |
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because atmospheric pressure is lower |
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normal boiling point |
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the boiling point of a liquid at a pressure of 101.3 kPa |
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What happens inside a solid structure when it is heated? |
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particles move more rapidly |
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What water is exactly at 0 degrees Celsius will it be a solid or liquid? |
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neither, it is in equilibrium |
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Most solid substances are ... |
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crystalline |
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crystalline |
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an orderly, repeating 3D pattern |
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unit cell |
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the smallest group of particles within a crystal that retains the geometric shape of the crystal |
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three basic types of unit cells |
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simple cubic body-centered face-centered |
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allotropes |
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solid substances that can exist in more than one form (same element) |
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3 different allotropes of carbon |
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diamond graphite buckyballs |
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amorphous solid |
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it lacks an ordered internal structure (eg rubber) |
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sublimation |
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state change directly from solid to gas |
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How is energy stored in a chemical? |
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in its chemical bonds |
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heat |
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energy that transfers from one object to another because of a temperature difference between the objects |
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heat vs. temperature |
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heat is the transferred energy temperature is a measure of heat |
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Law of Conservation of Energy |
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energy is neither created or destroyed in any physical or chemical process |
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heat capacity |
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amount of heat needed to increase the temperature of an object exactly one degree Celsius |
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heat capacity |
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amount of heat needed to increase the temperature of an object exactly one degree Celsius |
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specific heat capacity |
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amount of heat needed to increase temperature of 1 gram of a substance one degree Celsius |
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calorimetry |
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the measurement of heat flow into or out of a system for physical and chemical processes |
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q |
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heat |
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C |
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specific heat capacity of water |
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m |
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mass of water |
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delta T |
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change in temperature |
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molar heat of fusion |
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heat absorbed by one mole of solid substance as it melts to a liquid at a constant temperature |
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molar heat of vaporization |
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heat required to vaporize one mole of a given liquid at a constant temperature |
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phase diagram |
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shows relationship among pressure, temperature, and physical states of water |
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heating curve |
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graphically describes the enthalpy changes that take place during phase changes at a constant pressure |