For a thermodynamic data at 298k, when 2. 34 moles of nh3(g) react at standard conditions, the free energy change is mathematically given as
dG'−213.174KJ
Generally, the equation for the Chemical Reaction is mathematically given as
HCL+NH3----->NH4Cl
Therefore
dG=-202.9-[-16.5+(95.3)]
dG=-91.1KJ/mol
In conclusion, For 2.34 moles
dG'=-91.1KJ/mol*2.34
dG'−213.174KJ
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The free energy change when 2.34 moles of NH₃(g) react at standard conditions is -213.174 kJ.
Free energy change of any chemical reaction will be calculated by using the following chemical reaction:
ΔG = Free energy of products - Free energy of reactants
Given chemical reaction is:
NH₃ + HCl → NH₄Cl
From the stoichiometry of the reaction it is clear that same moles of ammonium chloride is produced by the same moles of ammonia & hydrochloric acid.
Free enrgy of NH₄Cl = -202.9 kJ/mol
Free enrgy of NH₃ = -16.5 kJ/mol
Free enrgy of HCl = 95.3 kJ/mol
On putting values in the above equation, we get
ΔG = -202.9-[-16.5+(95.3)]
ΔG = -91.1KJ/mol
For 2.34 moles, ΔG will be:
ΔG = (2.34)(-91.1) = -213.174 kJ
Hence required amount of free eenrgy is -213.174 kJ.
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