Chapter 6 – Chemistry – Flashcards
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| compressibility |
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| the chamge in volume resulting from a pressure change |
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| thermal expansion |
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| the change in volume resulting from temperature changes |
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| how does a thermometer work? |
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| 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. |
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| density of a solid |
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| high |
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| shape of a solid |
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| definite |
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| compressibility of a solid |
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| small |
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| thermal expansion of a solid |
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| very small |
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| density of a liquid |
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| high-usually lower than the corresponding solid |
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| shape of a liquid |
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| indefinite |
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| compressibility of a liquid |
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| small-usually higher than that of the corresponding solid |
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| thermal expansion of a liquid |
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| small |
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| density of a gas |
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| low |
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| shape of a gas |
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| indefinite |
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| compressibility of gas |
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| large |
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| thermal expansion of a gas |
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| moderate |
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| the kinetic molecular theory of matter is used to explain |
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| the behavior of matter in its various states |
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| first postulate of the KMT |
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| matter is composed of tiny particles called molecules |
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| second postulate of the KMT |
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| the particles are in constant motion and therefore possess kinetic energy |
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| third postulate of the KMT |
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| the particles possess potential energy as a result of attracting or repelling each other |
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| fourth postulate of the KMT |
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| the average particle speed increases ass the temperature increases |
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| fifth posulate of the KMT |
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| the particles tansfer energy to each other during collisions in which no net energy is lost from the system |
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| What makes a substance a solid liquid or gas |
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| itdepends on the strength of attractive foreces active between atoms. |
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| what unit is used for the volume of a solid |
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| centimeters cubed |
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| what unit will be used for volume of a gas? |
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| liters cubed |
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| unit for volume of a liquid? |
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| mL |
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| exact density is dependant on |
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| temperature |
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| two types of energy |
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| kinetic and potential |
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| potential energy |
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| stored energy |
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| kinetic energy |
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| energy of motion |
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| formula for kinetic energy |
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| one half times mass times velocity squared |
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| energy can be transformed from one type to another but cannot |
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| be created or destroyed |
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| six forms of energy |
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| heat, light, chemical, electrical, mechanical, nuclear |
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| Kinetic molecular theory of gases (1) |
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| consists of many particles (atoms or molecule) motion is random no attractive forces |
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| kinetic molecular theory of gases (2) |
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| space betweeen particles very large compared to size of particles |
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| Kinetic molecular theory of gases (3) |
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| kinetic energy of average particle proportional to temperature in kelvins |
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| kinetic molecular theory of gases (4) |
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| energy total after collsions results in NO loss of kinetic energy |
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| kinetic molecular theory of gases is based on the assumpts for |
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| ideal gases |
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| Three factors that are involved (when amount of gas is kept constant) |
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| pressure, volume, temperature (kelvins) |
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| when doing experiments you want to have only a single |
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| variable |
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| pressure |
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| the result of collisions of particles with sides of containers |
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| the more frequent and stronger the collisions of particles |
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| the higher the pressure |
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| psi |
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| pressure per unit area (pounds per square inch) |
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| Conversion factor from atm to mmHg |
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| 1 atm = 760 mmHg |
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| conversion factor from psi to atm |
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| 1 atm = 14.7 psi |
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| conversion factors from atm to torr |
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| 1 atm = 760 torr |
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| conversion factor atm to bars |
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| 1 atm = 1.01 bars |
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| conversion factor from kPal to atm |
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| 1 atm = 101 kPal |
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| is temperature the same thing as heat? |
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| no |
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| heat is a form of |
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| energy |
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| temperature can tell you the direction of |
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| energy (heat) flow |
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| absolute zero |
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| 0 kelvin |
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| what happens at absolute zero? |
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| all motion stops...particles have NO kinetic energy |
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| water freezing and boiling point (F) |
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| 32, 212 |
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| water freezing and boiling point in celsius |
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| 0, 100 |
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| water freezing and boiling point in kelvins |
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| 273.15, 373.15 |
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| boyles law involves the relationship between |
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| volume and pressure |
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| the higher the pressure |
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| the lower the volume |
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| boyles equation |
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| P1 V1 = P2 V2 |
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| Charles law involves the relationship between |
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| volume and temperature |
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| the higher the temperature |
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| the higher the volume |
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| in charles law, what is constant |
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| pressure |
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| law of gay-lussac involves the relationship between |
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| temperature and pressure |
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| combined gas law |
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| work when the amount of gas is fixed and the conditions are changed. |
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| avogadros law involves the relationship between |
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| moles of gas and volume |
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| when pressure and temperature are constant |
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| volume of a gas is directly proprtional to number of moles of gas |
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| STP |
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| standard temperature and pressure zero degrees C (273.15k) and 1 atm (760 mmHg) |
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| standard molar volume |
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| 22.4l/mol |
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| avogadros law (equation) |
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| PV=nRT |
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| A.L. P stands for |
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| pressure in atmospheres |
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| A.L. V stands for |
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| volume in liters |
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| A.L. T stands for |
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| temperature in kelvins |
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| A.L. n stands for |
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| number of moles |
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| A.L. R stands for |
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| 0.0821 L atm/mol k universal gas constant |
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| daltons law deals with |
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| total and partial pressure |
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| partial pressures of individual components are additive because |
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| the particles do not interact |
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| grahams law is the relationship between |
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| diffusion rate and molecular weight |
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| heat energy units |
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| joules or calories |
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| one calorie equals |
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| 4.138 Joules |
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| endothermic |
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| heat taken in (melting, boiling, sublimation) |
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| exothermic |
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| heat given off (freezing, condesation, deposition) |
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| describe the position and relationship of particles in liquid |
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| they are in constant motion but are constantly in contact with other molecules |
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| when particles have enough energy |
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| molecules can break free of others and go from the liquid to gas phase (overcome intermolecular forces) |
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| vapor |
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| the gas molecules in equilibrium with a liquid |
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| in evaporation, the molecules disperse because |
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| there is no closed container |
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| vapor pressure |
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| the partial pressure of gas molecules in equilibrium with the liquid |
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| vapor pressure is dependant on what two factors? |
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| identity of the liquid and teh temperature |
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| is vapor pressure a physical or chemical property? |
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| physical |
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| what is the relationship between vapor pressure and intermolecular forces operating |
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| they are inversly related |
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| the stronger the intermolecular forces the (blank) the vapor pressure |
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| lower |
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| what happens when vapor pressure equals atmospheric pressure what happens? |
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| the liquid boils |
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| the boiling point is dependant on |
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| atmospheric pressure |
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| melting point |
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| temperature at which a solid changes to a liquid |
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| sublimation |
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| solid changes directly into a gas withour going through the liquid phase |
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| problems involving temperature chage but no phase change need to take what into account? |
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| specific heat |
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| specific heat |
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| amounf of heat it takes to raise the temperature of 1 gram of a substance one degree |
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| Heat = |
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| specific heat times mass times temp change |
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| units used for specific heat |
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| joules per gram degrees celcius or calories per gram degrees celcius |
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| which has a higher specific heat, water or metal |
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| water |
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| heat of fusion |
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| quantity of head required to completely melt a substance once it has reached its melting point |
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| heat of vaporization |
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| quantity of heat needed to vaporize a liquid once it has reached its boiling point |
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| when a substance is melting or boiling, the temperature |
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| is constant |
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| when doing change of state problems, each step will be one of two teypes of problems: |
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| specific heat or phase change |
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| Daltons law deals with |
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| partial pressure |
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| partial pressures of individual components are additive because |
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| the particles do not interact |
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