Thermodynamics

Question 0

Reaction speed

Answer 0

How fast the reaction occurs

Question 1

Spontaneous reaction

Answer 1

Reaction that occurs without outside intervention

No heating, no current, no catalyst

Question 2

Entropy

Answer 2

A thermodynamic function that increases with the number of energetically equivalent ways to arrange the components of a system to achieve a particular state
S=k*ln(W)

Question 3

The second law of thermodynamics

Answer 3

Given work in a closed system, the final state will always have less potential energy than the initial state

Everything tends to a point of lowest stored energy

Which means, for any spontaneous process, the entropy of the universe increases
Also that thermal energy cannot travel from a cold area to a warm area
And finally, in any closed system, the entropy of the system will either remain constant or increase, but never decreases

Question 4

State function

Answer 4

The value depends on the state of the system

Question 5

Entropy (S) by state

Answer 5

Gas> liquid> solid

Question 6

Entropy of the universe

Answer 6

ΔHuniv=ΔHsys+ΔHsurr

Question 7

Gibbs free energy

Answer 7

The amount of work that can be done from the available energy in a system
ΔG= ΔH -T(ΔS)

Question 8

Zeroth law of thermodynamics

Answer 8

If two systems are each in thermal equilibrium with a third, they are also in thermal equilibrium with each other.

If A=B, and B=C, then A=C

Question 9

First law of thermodynamics

Answer 9

The increase in internal energy of a closed system is equal to the difference of the heat supplied to the system and the work done by it: ΔU = Q - W

Which means that all energy is conserved, it cannot be created or destroyed, only transfered from one state to another

And by adding heat to the system, you either increase internal energy or you cause work to be done within the system

Question 10

Gibbs free energy from equilibrium constant

Answer 10

ΔG=-RTln(K)

Question 11

Gibbs free energy from standard cell potential

Answer 11

ΔG=-nFE.cell

Question 12

Enthalpy

Answer 12

Sum of the internal energy to its pressure and volume

H=E+PV

Question 13

Boltzman equation

Answer 13

S=k*ln(W)

Question 14

Work from entropy

Answer 14

Ln(W)=S/k

Question 15

Entropy of a gas

Answer 15

S=kh*P

Kh- henrys constant

Question 16

Total Gibbs free energy in non-standard conditions

Answer 16

ΔG=ΔG°+RTln(Q)

Question 17

Surroundings Entropy

Answer 17

ΔSsurr=-(ΔHsys)/T

Question 18

Heat of reaction (ΔH)

Answer 18

ΔH=Σ(n)ΔHf{of products}-Σ(n)ΔHf{of reactants}
Otherwise
ΔH=ΔE-w
Or 
ΔH=ΔG+T(ΔS)

Question 19

Observing a change in entropy (S)

Answer 19

See which state has a greater number of possible arrangements
Greater number of reactants/products or a decrease in temperature yields a greater entropy

Question 20

ΔS of Surroundings

Answer 20

Because the reaction occured, the number of possible arrangements for molecules outside the given system changes
ΔSsurr=-ΔHsys/T

Question 21

Relationships between ΔSsurr and ΔSsys

Answer 21

One is positive while the other is negative

Differ by the ΔG

Question 22

ΔS of the universe

Answer 22

ΔSuni=ΔSsurr+ΔSsys

Question 23

Thermodynamic properties of spontaneous reactions

Answer 23

Whenever ΔSuniv (so ΔSsys+ΔSsurr) is positive,

The reaction is spontaneous

Question 24

Third law of thermo dynamics

Answer 24

As a system approaches absolute zero the entropy of the system approaches a minimum value and it is therefore impossible to reduce any system to absolute zero in a finite series of operations. The entropy of a perfect crystal of an element in its most stable form tends to zero as the temperature approaches absolute zero.

Question 25

Work

Answer 25

The use of energy to create a force Given in NewtonMeters, the product of force and displacement or the integral of Force as a function of displacement when graphed against eachother W=F*Δs=∫F(Δs)