Thermodynamics Flashcards

1
Q

First Law of Thermodynamics

A

Heat and energy are not created nor destroyed

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2
Q

Second Law of Thermodynamics

A

If the forward reaction is spontaneous, then the reverse reaction cannot also be spontaneous

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3
Q

Standard Conditions

A

Pressure at 1 atm
Solid and Liquids in pure state
298 K or 25 C
Energy of Formation = 0

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4
Q

Enthalpy (ΔH)

A
Change in Heat over the reaction
ΔH (-) -> Reaction is exothermic
ΔH (+) -> Reaction in endothermic
ΔH= H(products-H reaction
ΔH= bonds broken- bonds formed
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5
Q

Hess Law

A

Apply whatever has been done in the reaction to the ΔH

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6
Q

Heat Capacity

A

C(p)= ΔH/ΔT

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7
Q

Specific Heat

A

The amount of heat required to raise 1 gram of substance 1 degree celcius
q= mcΔT

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8
Q

Entropy( ΔS)

A
  • Measures the randomness or disorder of the system,
    Solid> Aqueous >Liquid>Gas— Higher Entropy
    More moles—Higher Entropy
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9
Q

Gibbs Free Energy

A

ΔG (-) > Reaction is spontaneous

ΔG(+) > Reaction is not spontaneous

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10
Q

Gibbs Free Energy Calculation

A

ΔG=ΔH-TΔS

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11
Q

Standard Free Energy Change and Normal

A

ΔG= ΔGs +RTln(Q)=ΔGs+2.303RTlog(Q)

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12
Q

Standard Free Energy and the Equilibrium Constant

A

ΔG=-RTln(K)= -2.303RTlog(K)

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