Calculate an estimate of the pressure of Ar gas that must be applied above water

Question

Calculate an estimate of the pressure of Ar gas that must be applied above water's surface in order to produce a 1.1 M solution of dissolved Ar. Assume that the gas does not dissociate in or react with water and that its dissolution obeys Henry's Law.

Print Calculator Periodic Table Ebook Question 12 of 12 (1 point) The Henry's law constant of argon in water at 25°C is 1.4 x103 mol/(L atm). Calculate an estimate of the pressure of Ar gas that must be applied above water's surface in order to produce a 1.1 M solution of dissolved Ar. Assume that the gas does not dissociate in or react with water and that its dissolution obeys Henry's law. Number atm If methane were to be at the same pressure above water's surface, the concentration of dissolved CH4 would be 1.2 M. What is the kH value of CH4? Number mol/L atm

Explanation / Answer

Solution :-

Part 1

Pressure for the Ar gas = ?

KH = 1.4*10^-3 mol / L atm

Concentration c = 1.1 M

Formula

c= KH* P

therefore

P= c/kH

= 1.1 mol per L / 1.4*10^-3 mol per L atm

= 785.7 atm

So the pressure of the Ar gas needed 785.7 atm or we can round it to 786 atm

Part 2

Concentration of the CH4 = 1.2 M

Pressure = 785.7 atm

KH= ?

KH = c/ P

        = 1.2 mol per L /785.7 atm

        = 1.53*10^-3 mol / L atm

So the KH for the CH4 is 1.53*10^-3 mol per L atm

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