CHEM 1312 Lecture Notes - Lecture 3: Partial Pressure, Mole Fraction, Torr

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Solubility of solids may increase, decrease, or remain relatively constant with increasing temperature. Increase in temperature, shift equilibrium to the right. Shift to the right and more solute dissolves. Increase temperature and shift equilibrium to the left. Reaction moves to the right (occupies less volume and decreases pressure) Henry"s law: the solubility of gas ( c ) is directly proportional to the partial pressure, p, over the solution. The solubility of n2 in blood at 37 c and at a partial pressure of. 0. 80 atm is 5. 6 x 10 4 mol l 1. A deep-sea diver breathes compressed air with the partial pressure of n2 equal to 4. 0 atm. Assume that the total volume of blood in the body is 5. 0 l. Calculate the a(cid:373)ou(cid:374)t of n(cid:1006) gas released (cid:894)i(cid:374) liters at (cid:1007)7 c a(cid:374)d (cid:1005) atm) when the diver returns to the surface of the water, where the partial pressure of n2 is 0. 80 atm. lecture notes page 1.