Gen Chem. 2 - Chapter 19 : Spontaneous & Non spontaneous Reactions

Whack SHIT

Spontaneous Process

A process that occurs without ongoing outside intervention

the spontaneity of a chemical reaction

The direction and extent to which a chemical reaction proceeds

Entropy

Is a thermodynamic function that increase with the number of energetically equivalent ways to arrange the components of a system to achieve a particular state

S

K * ln (W) =

K

Boltsmann constant (the gas constant/avogardo’s number)

W

The number of energetically equivalent ways to arrange the components of the system

W increases

Entropy increases when

Macrostates

Defined by a given set of conditions of a system (ex. P, V, and T in an ideal gas system)

Microstates

The exact internal energy distribution among the particles at one instant

Remains constant

Macrostates

Always changing (like a snapshot of the system at a given instant in time)

Microstates

W (micro/macro)

The number of possible microstates that can result in a given macrostate

Highest entropy, greatest dispersal of energy

The state with the ______ ________ has the _______ _________ ___ ___________

Second Law of Thermodynamics

For any spontaneous process, the entropy of the universe increase (deltaS > 0)

state function

Entropy is a

delta S

= S(final) - S(initial)

Entropy increases

Phase transition from a solid to a liquid

Entropy increases

Phase transition from a solid to a gas

Entropy increases

Phase transition from a liquid to a gas

Entropy increaces

An increase in the number of moles of a gas during a chemical reaction

Translational energy

Energy that takes the form of straight-line motions of the molecules

Rotational energy

Energy that takes the form of rotations of the molecules

Delta S

Q(rev)/T(constant temperature)

Q(rev)

The heat exchanged with the surroundings in a reversible process

Reversible process

A process that reverses the direction upon a small change in some property(ex. Melting of ice when the ice and its surroundings are both at exactly 0 degrees celsius)

T

Temperature in K (must be constant throughout the change, isothermal)

Delta S (universe)

= Delta S (system) + delta S (surroundings)

Entropy of the universe must increase

For a process to be spontaneous, the

Exothermic process

Increases the entropy of the surroundings

Endothermic process

Decreases the entropy of the surroundings

Dependent on temperature

The increase of of delta S (surroundings)

Entropy of delta S (surroundings) decreases

Temperature increases

Q(surroundings)

= - Q(systems)

Delta S (surroundings)

(-delta Heat System)/ T

- delta H (system) (negative)

Increases the entropy of the surroundings

Delta H (system) (positive)

Decreases the entropy of the surroundings