Term
| The state of a substance depends on what two factors |
|
Definition
|
|
Term
| what four properties are commonly used to distinguish substances? |
|
Definition
| density, shape, compressibility, thermal compression |
|
|
Term
|
Definition
| the mass of a sample of matter divided by the volume of the same sample |
|
|
Term
|
Definition
| sometimes dependant on container and sometimes not, depending on the state of matter |
|
|
Term
|
Definition
| the chamge in volume resulting from a pressure change |
|
|
Term
|
Definition
| the change in volume resulting from temperature changes |
|
|
Term
| how does a thermometer work? |
|
Definition
| thermal expansion-as the temp of the liquid increases, it expands and fills more of the fine capillary tube on with the temp scale is engraved. |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| compressibility of a solid |
|
Definition
|
|
Term
| thermal expansion of a solid |
|
Definition
|
|
Term
|
Definition
| high-usually lower than the corresponding solid |
|
|
Term
|
Definition
|
|
Term
| compressibility of a liquid |
|
Definition
| small-usually higher than that of the corresponding solid |
|
|
Term
| thermal expansion of a liquid |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| thermal expansion of a gas |
|
Definition
|
|
Term
| the kinetic molecular theory of matter is used to explain |
|
Definition
| the behavior of matter in its various states |
|
|
Term
| first postulate of the KMT |
|
Definition
| matter is composed of tiny particles called molecules |
|
|
Term
| second postulate of the KMT |
|
Definition
| the particles are in constant motion and therefore possess kinetic energy |
|
|
Term
| third postulate of the KMT |
|
Definition
| the particles possess potential energy as a result of attracting or repelling each other |
|
|
Term
| fourth postulate of the KMT |
|
Definition
| the average particle speed increases ass the temperature increases |
|
|
Term
| fifth posulate of the KMT |
|
Definition
| the particles tansfer energy to each other during collisions in which no net energy is lost from the system |
|
|
Term
| What makes a substance a solid liquid or gas |
|
Definition
| itdepends on the strength of attractive foreces active between atoms. |
|
|
Term
| what unit is used for the volume of a solid |
|
Definition
|
|
Term
| what unit will be used for volume of a gas? |
|
Definition
|
|
Term
| unit for volume of a liquid? |
|
Definition
|
|
Term
| exact density is dependant on |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| formula for kinetic energy |
|
Definition
| one half times mass times velocity squared |
|
|
Term
| energy can be transformed from one type to another but cannot |
|
Definition
|
|
Term
|
Definition
| heat, light, chemical, electrical, mechanical, nuclear |
|
|
Term
| Kinetic molecular theory of gases (1) |
|
Definition
| consists of many particles (atoms or molecule) motion is random no attractive forces |
|
|
Term
| kinetic molecular theory of gases (2) |
|
Definition
| space betweeen particles very large compared to size of particles |
|
|
Term
| Kinetic molecular theory of gases (3) |
|
Definition
| kinetic energy of average particle proportional to temperature in kelvins |
|
|
Term
| kinetic molecular theory of gases (4) |
|
Definition
| energy total after collsions results in NO loss of kinetic energy |
|
|
Term
| kinetic molecular theory of gases is based on the assumpts for |
|
Definition
|
|
Term
| Three factors that are involved (when amount of gas is kept constant) |
|
Definition
| pressure, volume, temperature (kelvins) |
|
|
Term
| when doing experiments you want to have only a single |
|
Definition
|
|
Term
|
Definition
| the result of collisions of particles with sides of containers |
|
|
Term
| the more frequent and stronger the collisions of particles |
|
Definition
|
|
Term
|
Definition
| pressure per unit area (pounds per square inch) |
|
|
Term
| Conversion factor from atm to mmHg |
|
Definition
|
|
Term
| conversion factor from psi to atm |
|
Definition
|
|
Term
| conversion factors from atm to torr |
|
Definition
|
|
Term
| conversion factor atm to bars |
|
Definition
|
|
Term
| conversion factor from kPal to atm |
|
Definition
|
|
Term
| is temperature the same thing as heat? |
|
Definition
|
|
Term
|
Definition
|
|
Term
| temperature can tell you the direction of |
|
Definition
|
|
Term
|
Definition
|
|
Term
| what happens at absolute zero? |
|
Definition
| all motion stops...particles have NO kinetic energy |
|
|
Term
| water freezing and boiling point (F) |
|
Definition
|
|
Term
| water freezing and boiling point in celsius |
|
Definition
|
|
Term
| water freezing and boiling point in kelvins |
|
Definition
|
|
Term
| boyles law involves the relationship between |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| Charles law involves the relationship between |
|
Definition
|
|
Term
| the higher the temperature |
|
Definition
|
|
Term
| in charles law, what is constant |
|
Definition
|
|
Term
| law of gay-lussac involves the relationship between |
|
Definition
|
|
Term
|
Definition
| work when the amount of gas is fixed and the conditions are changed. |
|
|
Term
| avogadros law involves the relationship between |
|
Definition
|
|
Term
| when pressure and temperature are constant |
|
Definition
| volume of a gas is directly proprtional to number of moles of gas |
|
|
Term
|
Definition
| standard temperature and pressure zero degrees C (273.15k) and 1 atm (760 mmHg) |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| 0.0821 L atm/mol k universal gas constant |
|
|
Term
|
Definition
| total and partial pressure |
|
|
Term
| partial pressures of individual components are additive because |
|
Definition
| the particles do not interact |
|
|
Term
| grahams law is the relationship between |
|
Definition
| diffusion rate and molecular weight |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| heat taken in (melting, boiling, sublimation) |
|
|
Term
|
Definition
| heat given off (freezing, condesation, deposition) |
|
|
Term
| describe the position and relationship of particles in liquid |
|
Definition
| they are in constant motion but are constantly in contact with other molecules |
|
|
Term
| when particles have enough energy |
|
Definition
| molecules can break free of others and go from the liquid to gas phase (overcome intermolecular forces) |
|
|
Term
|
Definition
| the gas molecules in equilibrium with a liquid |
|
|
Term
| in evaporation, the molecules disperse because |
|
Definition
| there is no closed container |
|
|
Term
|
Definition
| the partial pressure of gas molecules in equilibrium with the liquid |
|
|
Term
| vapor pressure is dependant on what two factors? |
|
Definition
| identity of the liquid and teh temperature |
|
|
Term
| is vapor pressure a physical or chemical property? |
|
Definition
|
|
Term
| what is the relationship between vapor pressure and intermolecular forces operating |
|
Definition
| they are inversly related |
|
|
Term
| the stronger the intermolecular forces the (blank) the vapor pressure |
|
Definition
|
|
Term
| what happens when vapor pressure equals atmospheric pressure what happens? |
|
Definition
|
|
Term
| the boiling point is dependant on |
|
Definition
|
|
Term
|
Definition
| temperature at which a solid changes to a liquid |
|
|
Term
|
Definition
| solid changes directly into a gas withour going through the liquid phase |
|
|
Term
| problems involving temperature chage but no phase change need to take what into account? |
|
Definition
|
|
Term
|
Definition
| amounf of heat it takes to raise the temperature of 1 gram of a substance one degree |
|
|
Term
|
Definition
| specific heat times mass times temp change |
|
|
Term
| units used for specific heat |
|
Definition
| joules per gram degrees celcius or calories per gram degrees celcius |
|
|
Term
| which has a higher specific heat, water or metal |
|
Definition
|
|
Term
|
Definition
| quantity of head required to completely melt a substance once it has reached its melting point |
|
|
Term
|
Definition
| quantity of heat needed to vaporize a liquid once it has reached its boiling point |
|
|
Term
| when a substance is melting or boiling, the temperature |
|
Definition
|
|
Term
| when doing change of state problems, each step will be one of two teypes of problems: |
|
Definition
| specific heat or phase change |
|
|
Term
|
Definition
|
|
Term
| partial pressures of individual components are additive because |
|
Definition
| the particles do not interact |
|
|
