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AP Chemistry Chapter 5: Thermochemistry

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Section 1

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specific heat capacity

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Chemistry Science

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Mar 1, 2020

Cards (34)

Section 1

(34 cards)

specific heat capacity

Front

the amount of energy required to raise the temperature of one gram of a substance by 1ºC. a substance with a high specific heat capacity a long time to heat up and cool down. a substance with a low specific heat capacity takes a short time to heat up and cool down.

Back

Heat of Combustion

Front

the heat released or absorbed when 1 MOLE OF A SUBSTANCE is burned

Back

change in enthalpy

Front

∆H= ∆E + P∆V ∆H=H products- H reactants the change in enthalpy is the heat gained or lost for most reactions ∆H is very close to ∆E because P∆V is so small, ∆H≈∆E

Back

first law of thermodynamics

Front

energy is neither created nor destroyed

Back

work

Front

energy used to cause an object that has mass to move w=-P∆V expansion-work done by gas: +∆V, -w compression-work done on a gas: -∆V, +w

Back

Change in the internal energy

Front

∆E = Efinal - Einitial ∆E=q + w

Back

endothermic

Front

the system absorbs energy from its surroundings q+

Back

kinetic energy

Front

due to motion of the object

Back

Heat calculation equation

Front

q=m x C x ∆T

Back

law of conservation of energy

Front

-q=q+

Back

heat capacity

Front

the amount of energy required to raise the temperature of a substance by 1ºC

Back

energy

Front

the ability to do work

Back

the system and the surroundings

Front

the system is the part of the universe on which you focus your attention the surroundings includes everything else in the universe

Back

enthalpy diagram

Front

Back

exothermic

Front

the system releases energy to its surroundings q-

Back

molar Heat of Solution ∆Hsoln

Front

heat change caused by dissolution of one MOLE of substance

Back

calorimetry

Front

the accurate and precise measurement of heat change for chemical and physical processes

Back

1 calorie

Front

4.184 joules

Back

Heat of a reaction

Front

∆Hºrxn= n∑∆Hfº (products) - n∑∆Hfº(reactants)

Back

Hess's law

Front

if a reaction is carried out in a number of steps, ∆Hrxn for the overall reaction is the sum of ∆H for each individual step allows us to calculate the ∆Hrxn by summing up each step's ∆H

Back

for enthalpy a process is exothermic when

Front

∆H is negative

Back

for enthalpy a process is endothermic when

Front

∆H is positive

Back

thermochemistry

Front

is concerned with the transfer of energy that occurs during a chemical reaction or physical process

Back

rules for using Hess's Law

Front

1. if you flip an equation around you must multiply the heat of reaction b -1 2. if you multiply the equation by a coefficient, you must also multiply the heat of reaction by the same number

Back

enthalpy (H)

Front

the heat released or absorbed from a system at CONSTANT pressure the same as heat but at CONSTANT pressure H=E +PV

Back

internal energy

Front

the internal energy of a system is the sum of all kinetic and potential energies of all components of the system; we call it E E=KE + PE to hard to find so we find the change in internal energy: ∆E

Back

thermochemical equation

Front

a chemical equation that includes a numerical value of the energy being absorbed or released

Back

State Functions

Front

It depends only on the present state of the system, not on the path by which the system arrived at that state ex: The internal energy of a system is independent of the path by which the system achieved that state; therefore internal energy is a state function. energy is a state function

Back

calorimeter

Front

a device used to measure the absorption or release of heat in chemical or physical processes. very good insulators

Back

the truth about enthalpy

Front

1.enthalpy is an extensive property 2.∆H for a reaction in the forward direction is equal to the backwards reaction, but opposite in sign 3. ∆H for a reaction depends on the state of the products and the state of the reactants

Back

potential energy

Front

due to position or chemical composition ex: gasoline (chemical potential energy)

Back

heat

Front

energy used to cause the temperature of an object to rise energy the transfers from one object to another because of a temperature difference between them. heat flows from warmer to cooler objects

Back

enthalpy of reaction, or heat of reaction

Front

∆H

Back

the standard heat of formation

Front

the amount of heat given off or absorbed when ONE MOLE OF A COMPOUND is made from its elements at standard conditions (25ºC, 1 atm) ∆Hº the standard heat of formation of an element=o this includes the diatomics

Back