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Chemistry 1a > Ch 6 - Thermochemistry > Flashcards

Ch 6 - Thermochemistry Flashcards

1
Q

thermochemistry

A

the study of the relationships between chemistry and energy

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2
Q

Exothermic Reaction

A

a reaction that gives off energy to the surrondings

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3
Q

Energy

A

the capacity to do work

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4
Q

Work

A

the result of a force acting through a distance

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5
Q

heat

A

the flow of energy caused by temperature differences

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6
Q

energy VS heat/work

A

Energy - something an object possesses

Heat/work - ways objects exchange energy

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7
Q

kinetic energy

A

the energy associated with the motion of an object

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8
Q

thermal energy

A

the energy associated with the temperature of an object.

A type of kinetic energy based on the motion of atoms or molecules within a substance.

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9
Q

potential energy

A

the energy associated with the position or composition of an object.

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10
Q

chemical energy

A

the energy associated with the relative positions of electrons and nuclei in atoms and molecules.

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11
Q

law of conservation of energy

A

energy can neither be created nor destroyed.

It can be:

  1. Transferred from one object to another
  2. assume different forms(potential to kinetic to thermal etc)
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12
Q

System

A

the specific setup being examined.

Example: reactants in a flask or a hand warmer in winter.

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13
Q

Surroundings

A

The systems surroundings are everything with which the system can exchange energy.

Example: Chemicals in a beaker can react with the solution, the beaker, air, the table, etc

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14
Q

Kintetic Energy equation

A

KE = 1/2mv^2

KE = kinetic energy
m = mass
v = velocity(m/s)
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15
Q

Mass

A

kg

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16
Q

Velocity

A

m/s

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17
Q

Joule

A

Named for James Joule.

SI unit of energy.

1 J = (1kg)(m^2/s^2)

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18
Q

Kilojoule

A

often used instead of the joule.

1 kJ = 1000J

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19
Q

“c” calorie(cal)

A

1 cal = 4.184 J(exact)

A larger unit than the Joule.

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20
Q

“C” Calorie(Cal) or kilocalorie

A

This is a kilocalorie.

1 Cal = 1000 cal

or

1 kcal = 1000 cal

or

1 kcal = 4184 J

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21
Q

kilowatt-hour(kWh)

A

1kWh = (3.60)*(10^6) J

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22
Q

First law of thermodynamics

A

the total energy of the universe is constant.

The is no free lunch. Everything costs something.

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23
Q

internal energy(E)

A

the sum of the kinetic and potential energies of all of the particles that compose a system

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24
Q

State function

A

the value of internal energy depends only on the state of the system not on how the system arrived at that state.

Flying or climbing to 10,000 feet are different avenues but either way you are at 10,000 feet(the state)

the change in state function only accounts for the initial and final states and does not care how it got there.

25
State function formula
change of E(the internal energy) = E(final) - E(initial)
26
Chemical system state function
change of E(the internal energy) = E(products) - E(reactants)
27
Energy Flow between system and surroundings
change E(sys) = - change(surr) Whatever one loses the other gains the exact opposite of.
28
q(heat)
+ means system gained thermal energy - means system lost thermal energy
29
w(work)
+ means work done on the system - means work done by the system
30
change E(internal energy)
+ energy flows into the system - energy flows out of the system
31
Energy, work and heat
Change E = q(heat) + w(work) ``` + = energy into the system - = energy out of the system ```
32
Temperature
a measure of the thermal energy within a sample of matter
33
heat
a transfer of thermal energy
34
thermal energy
always flows from matter with high temperature to low
35
thermal equilibrium
the point in which heat transfer stops because the two systems are the same temperature
36
heat capacity (C)
An extensive property(dependent on the amount of matter) the quantity of heat in a system required to change its temperature by 1 degree C.
37
heat capacity formula
C = q/change in temperature = J/degree C
38
heat formula
q = (C)(change in temperature) ``` q = heat C = heat capactiy ```
39
Specific Heat
intrinsic property. the amount of heat required to raise the temperature of 1 gram of a substance by 1 degree C.
40
Specific Heat formula
Cs = (J/g)(degree C)
41
Molar Heat capacity
the amount of heat required to raise the temperature of 1 mole of a substance by 1 degree C.
42
Heat/temperature/amount relationship
q = (m)(Cs)(change in temperature) q = heat m = mass Cs = specific heat capacity(J/g*Celsius) Change in temperature(Tfinal - Tinitial)
43
Thermal Energy Transfer
Since Qmetal = -Qwater: | Mmetal)(Cs,metal)(change temperature,metal) = -(Mwater)(Cs,water)(change temperature,water
44
Pressure-Volume-Work
when a force is caused by a volume change against an external pressure.
45
Work Formula
w= F * D OR(based on force definition) w = (P*A)(D) ``` w = work F = force D = distance ```
46
Pressure formula
P = F/A ``` P = pressure F = Force A = area ```
47
Force formula
variation on pressure formula. F = PA ``` F = force P = pressure A = area ```
48
Work and Volume
w = P*A*Change in H change in V = A*(change in H) So: w = -(P)(change in V)
49
J to (L)(atm) conversion
101.3J = (1L)(atm)
50
Calorimetry
the measure of the thermal energy exchanged between the reaction(defined by the system) and the surroundings by observing the change in temperature of the surroundings.
51
Bomb Calorimeter
a piece of equipment designed to measure the change of E for combustion reactions. ensures the reaction occurs at a constant volume
52
Water Specific Heat
4.18J/(g*celcius)
53
Enthalpy(H)
the sum of its internal energy and the product of its pressure and volume. H = E + PV deltaH = deltaE+P*deltaV
54
Endothermic Reaction
a chemical reaction with a positive deltaH absorbs heat from its surroundings A cold pack absorbs heat from your skin.
55
Exothermic Reaction
a chemical reaction with a negative deltaH releases heat to its surroundings. A chemical hand warmer gives off heat to your skin.
56
Enthalpy of reaction or Heat of Reaction
extensive property. delta Hrxn. The amount of heat generated or absorbed when a chemical reaction occurs depends on the amounts of the reactants that actually react.
57
Coffee-cup calorimeter
measures enthalpy changes for chemical reactions in solutions. Qsoln = (Msoln)(Cs,soln)(delta T) Qrxn = -(Qsoln)
58
Calorimetry Summary
Bomb Calorimetry occurs at a constand volume and measures the deltaE for a reaction. Coffee-cup calorimetry occurs at a constant pressure and measures deltaH for a reaction.

Chemistry 1a (15 decks)

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