- #1

davidbenari

- 466

- 18

## Homework Statement

The molar fraction of methane dissolved in water can be calculated from Henrys constant which are: 4.131 atm at 25ºC and 5.771 atm at 50ºC.

(a) Determine if the dissolution process of methane in water is exothermic or endothermic, and calculate the value of the enthalpy of dissolution for methane in water.

## Homework Equations

##\Delta H_{ideal}=0##

##\Delta S_{ideal}=-nR\Bigg(\sum_i x_i lnx_i\Bigg)##

##H^{Excess}=n\xi RT x_A x_B##

##p=K_{Henry}X_A##

## The Attempt at a Solution

[/B]

I don't see any pattern in the constants provided. The fact that pressure increases with temperature doesn't reflect any information about the interactions between the different molecules, so I can't deduce anything about enthalpy.

I frankly have no idea what to do for this problem I find it impossible... :S

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