Can someone help me write the equations for henrys law and raoults law (not necessarily solve them) for this question please??

A 1 m^{3} volume of water at 25°C initially contains 40 mg L^{-1} dissolved O_{2} and 1200 mg L^{-1} dissolved CO_{2} in a closed vessel with a large gas space of 10 m^{3} above the water. The solution can be considered to be ideally dilute. The gas space initially contains air at ambient conditions (i.e., 25°C, 1 atm total pressure, P_{O2} = 0.21 atm). The air initially contains no CO_{2}.

The following information is known about the system:

· Henry's Law constant (on a mole fraction basis) for O_{2} in water = 4.35 x 10^{4} atm at 25°C.

· Henry's Law constant (on a mole fraction basis) for CO_{2} in water = 1638.5 atm at 25°C.

· Enthalpy of solution of CO_{2} in water = -18,800 J mol^{-1}.

· Enthalpy of solution of O_{2} in water = -15,400 J mol^{-1}

· Density of water = 1 kg L^{-1}.

Neglect the vapour pressure of water, determine the concentrations (in units of mg L^{-1}) of dissolved O_{2} and CO_{2} remaining in solution when equilibrium between the two phases is reached at 25°C.

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