Answered

IDNLearn.com provides a comprehensive solution for all your question and answer needs. Our platform offers reliable and comprehensive answers to help you make informed decisions quickly and easily.

Arterial blood contains about 0.25 g of oxygen per liter at 37°C and standard atmospheric pressure. Under these conditions, the Henry's law constant is kH = 3.7 × 10^–2 mol/(L • atm), and the mole fraction of O2 in the atmosphere is 0.209

Calculate the solubility (in M) of O2 in the blood of a scuba diver at a depth of 100 feet, where Patm = ~3 atm

_______ M

Sagot :

The solubility (in M) of O2 in the blood of a scuba diver at a depth of 100 feet is 2.32 × 10^-3 mol.

How to calculate the solubility?

It should be noted that the partial pressure of oxygen will be:

= Mole fraction × Total pressure

= 0.209 × 3

= 0.627

According to Henry's law, the solubility will be:

= 3.7 × 10^-2 × 0.627

= 2.32 × 10^-3 mol

Learn more about blood on:

brainly.com/question/920424

#SPJ1

Thank you for using this platform to share and learn. Don't hesitate to keep asking and answering. We value every contribution you make. Your search for answers ends at IDNLearn.com. Thanks for visiting, and we look forward to helping you again soon.