This is my first term of chemistry and Iam having trouble wrapping my head aroun

Question

This is my first term of chemistry and Iam having trouble wrapping my head around this problem...

When a scuba diver is underwater the pressure of the air hebreathes increases in pressure. Determine the solubility of N2 in asolution (the diver’s blood) when exposed to an atmosphericpressure of 3.0 atm at 25°C while looking at a fish 66 ft belowthe sea level. Assume the mole fraction of N2 in their air supplyis 0.78. The Henry’s Law constant for N2 in H2O at this tempis 6.1x10^-4 M/atm.
Any help would be appreciated. This is my first term of chemistry and Iam having trouble wrapping my head around this problem...

When a scuba diver is underwater the pressure of the air hebreathes increases in pressure. Determine the solubility of N2 in asolution (the diver’s blood) when exposed to an atmosphericpressure of 3.0 atm at 25°C while looking at a fish 66 ft belowthe sea level. Assume the mole fraction of N2 in their air supplyis 0.78. The Henry’s Law constant for N2 in H2O at this tempis 6.1x10^-4 M/atm.
Any help would be appreciated.

Explanation / Answer

According to Henry's law,

solubility, c = kP

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