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
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