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Enthalpy of Solution vs Temperature

Enthalpy of Solution vs Temperature

Enthalpy of Solution vs Temperature

(OP)
Hello,
I am looking for a simple way to describe the dependence between the enthalpy of solution (e.g carbon dioxide (g) in hot water) and temperature.

Thanks in advance,

Mike

RE: Enthalpy of Solution vs Temperature

The enthalpy of solution is constant (or very close) for different temperatures.  What happens is as the CO2 is added, the temperature rise due to the heat of absorption cause the system temperature to rise.  As the sytemabsortion temperature rises, the equalibrium of CO2 in water drops and the CO2 will not absorb.  Once the solution is saturated with CO2, the temperature will stop rising because the is no more heat of solution.

RE: Enthalpy of Solution vs Temperature

(OP)
dcasto,

Thank you very much.

P.S. What is the sytemabsortion?

Regards,

Mike

RE: Enthalpy of Solution vs Temperature


The temperature dependence of the solubility of gases is given by the relation

dlnc/dT = ΔHsol/RT2

where c is the number of moles of gas dissolved in a definite volume of solvent and ΔHsol is the molar heat of solution, assumed constant in the given temperature interval.

Since values of c as function of T are amply tabulated, one could solve for the molar heat of solution from:
 
log(c2/c1) = - (ΔHsol/2.303R)(1/T2-1/T1)

2.303R can be replaced by 4.576, and T are in Kelvin.

RE: Enthalpy of Solution vs Temperature

As the system temperature...

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