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As a scuba diver descends under water, the pressure increases. At a total air pressure of 2.96 atm and a temperature of 25.0 C, what is the solubility of \rm N_2 in a diver's blood? [Use the value of the Henry's law constant K calculated in Part A, \rm 6.26\times 10^{-4}\;\rm mol/(L\cdot atm).]

Assume that the composition of the air in the tank is the same as on land and that all of the dissolved nitrogen remains in the blood.

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