Explain why the ΔH of sol for sodium chloride is favorable to the formation of an aqueous solution of sodium chloride?
NaCl(s) --> Na+(aq) & Cl- (aq)
dH reaction = dHf products - dHf reactants
dH rxn = [dHf Na+(aq) & dHf Cl- (aq)] - dHf NaCl(s)
dH rxn = [ -240.1 & -167.2] - (-410.9)
d Hrxn = +3.6 kJ/mol
sorry dH = "+" , & so is not favorable by dH
we know that it does dissolve & dissociate easily...
so dG must be = a "-"
and the only way that dG = "-"...... must be that dS is favorable
dS reaction = S products - S reactants
dS rxn = [S Na+(aq) & S Cl- (aq)] - S NaCl(s)
dS rxn = [ 59 & 56.5] - (72.33)
d Srxn = +43.17 joules /mol ... or 0.04317 kJ
well dS = "+" 's are favorable
lets go for the dG @ 25 Cesius, 298Kelvin:
dG = dH - TdS
dG = 3.6 kJ -(298K)(43.17 kJ)
dG = 3.6 kJ - 12.865 kJ
dG = - 9.26 kJ
so because the dG is "-"
and because the dS is "+"
this reaction is favorable
but with no thanks to a "+" dH which is unfavorable
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NaCl(s) --> Na+(aq) & Cl- (aq)
dH reaction = dHf products - dHf reactants
dH rxn = [dHf Na+(aq) & dHf Cl- (aq)] - dHf NaCl(s)
dH rxn = [ -240.1 & -167.2] - (-410.9)
d Hrxn = +3.6 kJ/mol
sorry dH = "+" , & so is not favorable by dH
we know that it does dissolve & dissociate easily...
so dG must be = a "-"
and the only way that dG = "-"...... must be that dS is favorable
NaCl(s) --> Na+(aq) & Cl- (aq)
dS reaction = S products - S reactants
dS rxn = [S Na+(aq) & S Cl- (aq)] - S NaCl(s)
dS rxn = [ 59 & 56.5] - (72.33)
d Srxn = +43.17 joules /mol ... or 0.04317 kJ
well dS = "+" 's are favorable
lets go for the dG @ 25 Cesius, 298Kelvin:
dG = dH - TdS
dG = 3.6 kJ -(298K)(43.17 kJ)
dG = 3.6 kJ - 12.865 kJ
dG = - 9.26 kJ
so because the dG is "-"
and because the dS is "+"
this reaction is favorable
but with no thanks to a "+" dH which is unfavorable