As a scuba diver descends under water, the pressure increases. at a total air pressure of 2.71 atm and a temperature of 25.0 c, what is the solubility of n2 in a diver's blood? [use the value of the henry's law constant k calculated , 6.26 x 10^{-4} (mol/(l*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. express your answer with the appropriate units.

Liquid ammonia is produced at high temperatures and under great pressure in a tank by passing a mixture of nitrogen gas and hydrogen gas over an iron catalyst. the reaction is represented by the following equation. n2(g) + 3h2(g) → 2nh3(g) changing all but one experimental condition will affect the amount of ammonia produced. that condition is a) increasing the concentration of both reactants b) changing the temperature within the tank c) decreasing the pressure within the tank. d) increasing only the amount of nitrogen present.