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At 37^(@)C and 0.80 atm partial pressure...

At `37^(@)C` and `0.80 atm` partial pressure, the solubility of `N_(2)` was found to be `5.6 xx 10^(-4) mol//L`. A deep sea diver breathes compresssed air with the partial pressure of `N_(2)` equal to `4.0 atm`. The total volume of blood in his body is `5.0` litre. After sometime he comes back on the water surface where `P'_(N_(2))` is `0.80 atm`. Calculate the volume of `N_(2)` escaped during his return from depth to surface, at `37^(@)C` and `1 atm P`.

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To solve the problem step by step, we will follow the principles of Henry's Law and the Ideal Gas Law. ### Step 1: Calculate the Henry's Law constant (k_h) Given: - Solubility of \(N_2\) at \(0.80 \, \text{atm}\) = \(5.6 \times 10^{-4} \, \text{mol/L}\) According to Henry's Law: ...
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