Under high pn2 more nitrogen dissociates into blood the...

Under high $P_{N2}$ more nitrogen dissociates into blood. The bends occur when pressure decreases and nitrogen forms bubbles as it comes out of solution. If a patient breathes air highly concentrated in oxygen (as in a hyperbaric chamber), a high 1. Boyle's law percentage of oxygen will dissolve in the blood and 2. Dalton's law tissues. This is the principle underlying the use of a 3. Henry's law hyperbaric chamber. The total atmospheric pressure (760 mm Hg) is due mostly to pressure caused by nitrogen, partly to $P_{O2}$ and slightly to $P_{CO2}$. As the size of the thorax increases, pressure within it decreases.

Transcript

0:00 Hello.

00:01 So in this question we have to find, we are given some information and we have to find the moles of nitrogen and also the volume of the nitrogen and also the henry's constant.

00:17 So, so first that to find the moles of nitrogen in one liter blood at one atmospheric pressure.

00:24 So we know that that the solubility of nitrogen, it is given that is 0 .015 gram per liter.

00:37 So that means 0 .015 gram of nitrogen, it is present in 1 liter of blood.

00:52 Therefore, the mass of nitrogen gas in 1 litre of blood is equal to 0 .015 gram.

01:10 So we know that the molar mass of nitrogen, it is, for 1 nitrogen it is 14, 2 nitrogen atom it is there, that is 2 multiplied by 14 is equal to 28 gram per mole is the 1.

01:24 Molar mass.

01:25 Now we can calculate we have the mass and we have the molar mass.

01:29 Now it is easy to calculate the moles of the nitrogen gas because we know that number of moles for nitrogen gas is equal to mass of nitrogen.

01:47 We know that mass is equal to mass upon molar mass.

01:50 So here the moles for nitrogen get it is equal to mass of nitrogen.

01:54 Of nitrogen divided by molar mass of nitrogen here.

02:00 So we have the value 0 .015 divided by 28 and hence it will become 0 .000 536 moles are there and therefore we can say that in one liter blood in one liter blood at one at one atmospheric pressure, the moles of nitrogen, it is equal to, we can convert it in a standard form that is 5 .36 multiplied by 10 raised to the power minus 4 mole.

02:42 Hope this is clear to you.

02:44 Now, now we have to find the number of moles of nitrogen in one liter blood at 1 -8, at 1 .8, at 1.

02:58 Atmospheric at 4 atmospheric in 100 feet depth.

03:12 We know that air has 78 % of nitrogen.

03:20 That means 78 mole of nitrogen it is present in 100 mole of air.

03:30 We can say that regarding this statement.

03:34 So therefore therefore the moles of nitrogen is equal to 78 mole and moles of air is equal to 100 moles.

03:50 So, mole fraction for this nitrogen gas, it will be the moles of nitrogen divided by moles of air.

04:03 Mean 78 is present in 100.

04:07 So it will be 0 .78 in this case.

04:11 Now the partial pressure, partial pressure of n2, it can be calculated at one atmospheric as the mole fraction for nitrogen multiply by partial pressure of total partial pressure.

04:29 So as we know that this value, it is 0 .78 multiplied by and it is considered at one atmospheric pressure.

04:37 Therefore the partial pressure of nitrogen, it is 0 .78 atmospheric for this one.

04:48 Now according to henry law, it states that henry's law, it states that that partial pressure of nitrogen is equal to concentration of dissolved gas multiply by henry's constant.

05:10 This p, n2, it is a partial pressure of the n2.

05:14 And we know the value that is 0 .78.

05:17 And the concentration of dissolved gas, it is 5 .36 multiplied by 10 raised to the power minus 4 mole per liter.

05:27 And the k value, that is a henry's constant that we have to find out.

05:34 So here we can say that the value of k, it is, it will be 0 .78 multiplied by 5 .36 multiplied by 10 raised to the power minus 4...

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