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Chem 112 > Chapter 6 > Flashcards

Chapter 6 Flashcards

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1
Q

How is energy transferred?

What is it?

A

Through heat

The flow of energy caused by a temperature difference

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2
Q

What is chemical energy?

A

The energy associated with the relative positions of electrons and nuclei in atoms and molecules
Form of potential energy

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3
Q

What is the system in energy?

A

The system is the object with the energy initially

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4
Q

What is the surrounding in energy?

A

Are everything with which the system can exchange energy

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5
Q

What is the formula using mass velocity and kinetic energy?

A

KE= 1/2 mv^2

M in kg
V in m/s
KE in J

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6
Q

What are thermodynamics?

A

The general study of energy and its interconversions

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7
Q

What is the first law of thermodynamics?

A

The total energy of the universe is constant

The universes energy content does not change since energy cannot be created more destroyed

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8
Q

What is internal energy? Is it a state function?

A

E

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

Yes it is a state function since it depends only on the state of the system

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9
Q

What is the internal energy equation?

A

TriangleE= Efinal- Einitial

Or

               Eproducts-EReactants
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10
Q

How does the internal energy of the surrounding compare to the energy of the system?
Is this the same for heat?

A

TriangleEsystem= -triangleESurroundings

Yes,
Qsystem=-Qsurroundings

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11
Q

When the system is positive where does energy flow?

A

Into the system from the surroundings

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12
Q

What is the equation of the internal energy involving work and heat transferred?

A

TriangleE=q+w

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13
Q

What is heat?

What’s temperature?

A

The exchange of thermal energy between a system and its surroundings caused by a temperature difference

Temperature is a measure of the thermal energy in a sample

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14
Q

Where does thermal energy always flow?

A

From matter at high temperatures to matter at lower temperatures

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15
Q

What is the formals using heat, heat capacity and change in temperature?
How about using specific heat capacity?

A

Q=C (TriangleT)
q= heat
C= heat capacity
Triangle T= change in temp

q=m x Cs x triangleT

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16
Q

What’s the difference between heat capacity, specific heat capacity, and molar heat capacity?

A

Heat- heat required to raise temp by 1 degree C
Specific Heat- heat required to raise 1 gram of substance by 1 degree C (J/g•C)
Molar heat- heat required to heat 1 mole of substance by 1 degree C (J/mol•C)

17
Q

What is the equation for work, pressure and change in volume?

A

w=-PtriangleV
P= external pressure
V= litres

18
Q

What is the heat at a constant volume equation?

A

🔺Erxn=qv+w
W=0 at co stang volume so
🔺Erxn=qv

19
Q

What is the equation to find heat using a bomb calorimeter? What’s the equation if no heat escapes from the calorimeter?

A

qcal=Ccal • 🔺T
Ccal= heat capacity of entire calorimeter assembly

qcal=-qrxn

20
Q

What is enthalpy?

What’s its formula?

A

The sum of a systems internal energy and the product of its pressure and volume

H= E + PV

🔺H=🔺E+P🔺V
🔺H=(Qp+w) + (-w)
🔺H=Qp (the heat at constant pressure)

21
Q

What is an endothermic reaction compared to an exothermic one?

A

Endothermic- absorbs heat from its surroundings (🔺H is positive)
Exothermic- gives off heat to its surrounding (🔺H is negative)

22
Q

What are the three rules with Hess’s law involving 🔺Hrxn?

A
  1. If the chemical equation is multiplied by some factor then 🔺Hrxn is also multiplied by the same factor
  2. If the equation is reversed then 🔺Hrxn changes sign
  3. If the equation can be expressed as a sum of steps then the 🔺Hrxn is the sum of the heats for those steps
23
Q

What’s is the standard state for enthalpy?

For gas, liquids and solids, and substance in a solution

A

Gas- pure gas at pressure 1 atm
Liquid or solid- pure substance at 1 atm and at temp of interest (25C)
Substance in a solution- concentration of 1M

24
Q

What is the standard enthalpy change ( 🔺Hdegree)

A

Change in enthalpy for a process when all reactants and products are in their standard states
Degree sign indicates standard states

25
Q

What is the enthalpy of formation?
(🔺Hdegree f)
For a pure compound and a pure element in standard state

A

Pure compound- change in enthalpy when 1 mole of compound forms into constituent elements is standard state
Pure element in its standard state- 🔺Hdegree f= 0

26
Q

What is the formula for calculating the standard enthalpy change for a reaction?

A

Reactants -> elements 🔺H1=-Ē🔺Hdegree f (reactants)
Elements -> products 🔺H2= +Ē🔺Hdegree f (products)

= reactants -> products 🔺Hrxn=🔺H1+🔺H2

Chem 112 (11 decks)

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