Assume that argon exerts a partial pressure of 6 bar. Calculate the solubility of argon gas in water. (Given Henry’s law constant for argon dissolved in water, `K_(H)` = 40kbar)

Solubility of a gas in water is 0.001 m at STP, determine its Henry's law constant.

At what partial pressure , oxygen will have a solubility of 0.06 gL^(-1) in water at 298 K ? Henry's law constant (K_(H)) of O_(2) in water at 303 K is 46.82 k bar .(Assume the density of the solution to be the same as that of water).

If N_(2) gas is bubbled through water at 293 K , how many millimoles of N_(2) gas would dissolve in 1 L of water. Assume that N_(2) exerts a partial pressure of 0.987 bar. Given that Henry law constant for N_(2) at 293 K is 76.48 kbar.

Applying Henry's law: At 1.0 atm pressure, 24 g of acetylene (C_(2)H_(2)) dissolves in 1 L of acetone. If the partial pressure of acetylene is increased to 12 atm , what is the solubility in acetone? Strategy: Let S_(1) be the solubility of the gas at partical pressure P_(1) , and let S_(2) be the solubility at partial pressure P_(2) . Writing Henry's law for both pressure, we have S_(1)=KP_(1) S_(2)=KP_(2) Dividing the second equation by the first, we get S_(2)/S_(1)=(KP_(2))/(KP_(1)) or S_(2)/S_(1)=P_(2)/P_(1) we can use this relation to find the solubility at one pressure given the solubility at another.

1 kg of water under a nitrogen pressure of 1 atmosphere dissolves 0.02 gm of nitrogenat 293 k. Calculate Henry' s law constant :