Thermochemistry Flashcards

1
Q

These conditions are 298K, 1atm, and 1M, and are NOT the same thing as STP

A

Standard conditions

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2
Q

It’s symbol is ΔH, and it refers to the amount of heat in a reaction, with negative being exothermic and positive behind endothermic

A

Standard enthalpy

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3
Q

It’s symbol is ΔS, and it refers to the amount of chaos or the spread of molecules in a reaction

A

Standard entropy

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4
Q

It’s symbol is ΔG, and it refers to the amount of energy released in the conversion of reactants to products

A

Standard free energy change

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5
Q

What is the difference between a state process and a process function?

A

A state function describes a system in equilibrium, but doesn’t describe the pathway it took to get there (ex: density, pressure, Gibbs free energy)

A process function describes the pathway a reaction takes from 1 equilibrium state to another (ex: heat and work)

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6
Q

According to Hess’s Law, changes in enthalpy are _____, so no matter what path a reaction takes, it will end up with the same change in enthalpy

A

Additive

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7
Q

What is the equation for Gibbs free energy? (at standard conditions)

A

ΔG=ΔH-TΔS

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8
Q

Gibbs free energy outcomes:

ΔH +
ΔS +

A

Spontaneous only at high temps

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9
Q

Gibbs free energy outcomes:

ΔH +
ΔS -

A

Nonspontaneous at all temps

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10
Q

Gibbs free energy outcomes:

ΔH -
ΔS +

A

Spontaneous at all temps

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11
Q

Gibbs free energy outcomes:

ΔH -
ΔS -

A

Spontaneous at low temps

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12
Q

A reaction is spontaneous if ΔG is _____ and non spontaneous if ΔG is ____

A

Negative

Positive

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13
Q

Equation for Gibbs free energy at non-standard conditions

A

ΔGrxn= ΔG+RTlnQ

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