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Q
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Free energy
Gibbs or free energy used in thermodynamic chemistry for calculating the
reversible work at stable temperature and pressure or free energy is equal to the
change in enthalpy that subtract with change in entropy and temperature in kelvin
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free energy means the
maximum work done of the system which is performed by the
surroundings that underwent in the spontaneous changes
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In ideal gases, V is changed via the nRT/p is equivalent to the free energy
and the final and initial pressures are also involved;
∆G = (nRT/ P)∆P

nRT

∆𝑃
𝑃

= nRTln (Pf/Pi)

When the initial condition is standard with Pi is equivalent to the 1atm then change
in free energy can be written as following;
G – GO = nRTln P
G = GO + nRTln P

Or

Kp and K is used as a various equilibrium constants that is used for various units
so, in these equations this can be written with relation to ∆𝐺 and Kp
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When the ∆Go is greater than zero then the Kp
is smaller than one then the reactants are more favored against the products
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Since, Kp means that at equilibrium constant, partial pressures of the reactants and
products while on the other hand K refers as the amounts of products and reactants
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of moles of the gases’ products that
subtract the no
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In the reactions which contain solids or
liquid then ∆n is equivalent to zero while the Kp is equal to the K
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Negative
sign represented that in spontaneous reaction whether the reaction is forward or
backward
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When the ∆Go is positive then the log of K should be negative or less than 1, the
spontaneous reaction will proceed in reversed
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Entropy
Entropy have great significance in the thermodynamic chemistry that is the
measurement of the system’ thermal energy which is unattainable to doing
work or it is the disorder in the system
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S = kb ln Ω
In which the S is equivalent to the entropy, kb is known as the Boltzmann
constant, ln is the logarithm and Ω is the no
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Solids have less property than others states due to the
arrangement is randomness or very little
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In the Gibbs energy equation, the entropy is used and possess relation;
∆G = ∆𝑯 + T∆S
So, Gibbs free energy contain the relation with equilibrium
∆GO = -RTln K
Or,
-∆Go / R = T log K
So, in reversible reaction the equilibrium with surrounding is that;
∆S = 0, ∆SS = ∆Ssurrounding
𝒂𝒕 ∆GO = 0
𝑺𝒐, That
∆H = T∆SS = -T∆SSurr
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- T∆Ssys
= -T (∆SSurr
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Endothermic means that heat lose via the surroundings to the
system which causes the entropy to become lowers of the surroundings
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The Gibbs free energy is equal to the;
∆G = ∆H - T∆S
RTln Keui = ∆H - T∆S
RTln Kequi = -T∆S



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