Respuesta :
The free Gibbs energy ΔG for a given chemical reaction is -33kJ.
Gibbs free energy: What does it mean?
The Gibbs free energy, also referred to as the Gibbs function, Gibbs energy, or free enthalpy, is a unit of measure for the maximum amount of work carried out in a thermodynamic system under constant temperature and pressure. The letter "G" stands for Gibbs free energy.
Given equation.
N₂ + 3H₂ → 2NH3
Formula for finding change in gibbs free energy of a chemical reaction is as follows
ΔG = ΔH - TΔS
Where
ΔH = change in enthalpy
ΔS = change in entropy
T = absolute temperature
Given chemical reaction of nitrogen and hydrogen is
N₂ + 3H₂ → 2NH3
According to the value slipped in thew table from the back book, ΔH for H₂ and N₂ is zero and ΔH for NH₃ = -46.11kJ
ΔH (2NH₃) = 2(-46.11)
ΔH (2NH₃) = -92.22kJ
According to the value slipped in thew table from the back book the entropy value for N₂ is SN₂ = 192.61J/k
H₂ is SH₂ = 3( 130.68J/k)
NH₃ is SNH₃ =192.45J/k
So the change in entropy for the chemical reaction is,
ΔS = [(2×192.45) - (191.61) - (3×130.68J/k)]
ΔS = 384.9 - 191.61 - 392.04
ΔS = -198.75J/k
The amount of heat that can go out of the system
TΔS = (298k) (-198.75J/K)
TΔS = - 59.23 kJ
Substitute - 59.23 kJ for TΔS and - 92.22kJ for ΔH
ΔG = ΔH - TΔS
ΔG = -92.22kJ - (-59.23kJ)
ΔG = -33kJ
Free Gibbs energy ΔG for a given chemical reaction is -33kJ.
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