Asked by Raoul
The enthalpy of solution of nitrous oxide (N2O) in water is -12 kJ/mol and its solubility at 20 oC and 1.00 atm is 0.121 g per 100. g of water. Calculate the molal solubility of nitrous oxide in water at 1.600 atm and 20 oC. Hint, first find Henry's law constant at 20 oC and 1.00 atm.
Answers
Answered by
DrBob222
I suppose you are to use M and m as the same.
0.121g/100 gH2O = solubility.
mol N2O = 0.121/60 = approx o.002 and 0.002/0.1kg solvent = 0.02m
p = KcC
1 atm = Kc*0.02
Kc = 1 atm/0.02 = 50 atm/m
p = KcC
1.600 = Kc from above *C
Solve for C in molality and convert to g/100 if desired.
0.121g/100 gH2O = solubility.
mol N2O = 0.121/60 = approx o.002 and 0.002/0.1kg solvent = 0.02m
p = KcC
1 atm = Kc*0.02
Kc = 1 atm/0.02 = 50 atm/m
p = KcC
1.600 = Kc from above *C
Solve for C in molality and convert to g/100 if desired.
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