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To simulate Natural gas mixture over water, 10 moles of methane (CH4) and 1 mole of...

To simulate Natural gas mixture over water, 10 moles of methane (CH4) and 1 mole of ethane (C2H6) were injected into a 30.0 L cylinder at a temperature of 30.0 oC? One third of this cylinder is filled with water so remaining volume is left for the binary gas mixture. Answer the following: (i) Calculate mole fractions Xmethane and Xethane ? Hence calculate the, (a) molar Gibbs free energy-change of mixing ΔGm? (b) molar entropy-change of mixing ΔSm? (ii)With both gases behaving ideally, calculate total pressure in atm using ideal gas law? (iii) Based on (i) & (ii) calculate the partial pressures PCH4 and PC2H6 in atm using Dalton’s law? (iv)According to Henry’s law related to gas solubility in water, [Cgas] = Pgas x HK(gas) where Pgas is the partial pressure of gas over water and [Cgas] is the concentration of gas in water. HK(gas) constant values of ethane and methane are listed in table below: Gas Methane (CH4) (mol/(L.atm) Ethane (C2H6) (mol/(L.atm) HK(gas) 1.23x10-3 1.61x10-3 *Find the concentrations in (mol/L) then (g/L) of CH4 and C2H6 gases in water?

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