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Chemistry studying

chapter 17 prentice hall- heat

Endothermic The system gains heat as the surroundings cool down (example: someone sitting my a campfire), defined as a positive q value specific heat specific heat of a substance is the amount of heat it takes to raise the temp of 1 gram of the substance 1 degree celsius.
Exothermic loses heat as the surroundings heat up. (Example: someone running and sweating), defined as a negative q-value because the system is losing heat how to convert from joules to calories? 1 joule= 0.239 cal and 4.184 J=1 calorie
Heat always flows from a warmer object to a cooler object. heat capacity depends on the mass and chemical composition of the object. it is defined as the amount of heat needed to raise the objects temp 1 deg celsius.
Heat flow measured in 2 common units: calories and the Joule. q=?,m=?,c=?,deltaT=? q=amount of heat, m=mass, c=specific heat of substance, deltaT= change in heat(final temp-initial temp)
Calorie defined as the quantity of heated needed to raise the temperature of 1 gram of pure water 1 degree Celsius. device used to measure absobation or release of heat in an experiment calorimeter
C,c C=dietary calorie (equals one kilocalorie/1000 calories). c=calorie enthalpy heat content of object at constant pressure AKA q (i think)
10g of sugar has 41 calories 10g of sugar releases 41 kilocalories of heat when completely burned heat of fusion h-delta-fus (the amount of heat absorbed by one mole of a solid substance as melts to a liquid)
Equation to find amount of heat Q=m•C•deltaT heat of vaporization amount of heat needed to vaporize 1 mole of a certain liquid
Hess's law determines the heat of reaction indirectly
Created by: lalamina