entropy and energetics

Question 1

equation for ΔS(total)

Answer 1

ΔS(system) + ΔS(surroundings)

Question 2

equation for ΔS(system)

Answer 2

S(products) - S(reactants)

Question 3

equation for ΔS(surroundings)

Answer 3

• ΔH/T

Question 4

equation for gibbs free energy

Answer 4

ΔH - TΔS(system)

Question 5

how to check if a reaction is thermodynamically feasible (spontaneous)

Answer 5

feasible if ΔG < 0

Question 6

what sign for ΔH means more stable products

Answer 6

-ve

Question 7

what sign for ΔS means more stable products

Answer 7

+ve

Question 8

bonds broken: C-O and O-H; bonds made: C-O and O-H; why is ΔH not zero

Answer 8

bond enthalpies differ between compounds

Question 9

state the relationship between ΔS(total) and equilibrium constant K

Answer 9

ΔS(total) = RlnK

Question 10

what is the unit of S

Answer 10

J K^-1 mol^-1 (joules per kelvin per mole)

Question 11

what is the point of finding ΔG

Answer 11

to see if a reaction is feasible (it converts units of ΔS(total) to J mol^-1 and swaps its sign for some reason)

Question 12

why is that the equation of ΔS(surroundings)

Answer 12

ΔS(surr) = - ΔH/T; it converts the ΔH(surroundings) ( equal to - ΔH(system) ) into the units of entropy