The suitable condition for the below transformation is: S. S condition [A] H0/1: (5 mol%)/H30 -B] H2O/Cl2 (5 mol %)/H2O [C] H2O2/F2 (5 mol%)/H2O @ [D] H:03/F: (20 mol%)/H2O
Answers
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Answer:
second law of thermodynamics to determine if a process is spontaneous is that we must determine the entropy change for the system and the entropy change for the surroundings. An alternative approach involving a new thermodynamic property defined in terms of system properties only was introduced in the late nineteenth century by American mathematician Josiah Willard Gibbs. This new property is called the Gibbs free energy change (G) (or simply the free energy), and it is defined in terms of a system’s enthalpy and entropy as the following:
G=H−TS
G
=
H
−
T
S
Free energy is a state function, and at constant temperature and pressure, the standard free energy change (ΔG°) may be expressed as the following:
ΔG=ΔH−TΔS
Δ
G
=
Δ
H
−
T
Δ
S
We can understand the relationship between this system property and the spontaneity of a process by recalling the previously derived second law expression:
Δ
S
univ
=
Δ
S
+
q
surr
T
ΔSuniv=ΔS+qsurrT
The first law requires that qsurr = −qsys, and at constant pressure qsys = ΔH, and so this expression may be rewritten as the following:
Δ
S
univ
=
Δ
S
−
Δ
H
T
ΔSuniv=ΔS−ΔHT
ΔH is the enthalpy change of the system. Multiplying both sides of this equation by −T, and rearranging yields the following:
−)