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Gnom [1K]
3 years ago
11

At a depth of 100 ft in water, the external pressure is 4.0 atm. What is the solubility of N2 from air in blood at this pressure

Chemistry
1 answer:
Ira Lisetskai [31]3 years ago
8 0

Answer:

Solubility  = 2.142 x  10^{-4} M

Explanation:

Solution:

Note: This question is incomplete and lacks necessary data to solve this question. But I have found similar question on the internet and fetched the necessary data to solve:

Missing Data:

Number of Moles of N2 dissolved per litre of blood = 5.357 x 10^{-4} M

As we know that, the air is approximately. 78 mol % of N2

N2 = 0.78

Partial pressure of the N2 at 100 ft:

Partial Pressure = 0.78 x (4.0)

Partial Pressure = 3.12 atm

Now, this is 4 times the pressure of nitrogen at 1 atm air pressure.

SO,

According to the Henry's Law, we have:

Solubility = k x P_{g}

Here, k = 4 times

So,

Solubility = 4 x (5.357 x 10^{-4})

Solubility  = 2.142 x  10^{-4} M

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3 0
2 years ago
Changing the number of protons in an atom makes<br><br> A. an ion<br> B. an isotope
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With reference to He-4 (or the diagram), explain the term isotopes.
boyakko [2]

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6 0
3 years ago
At equilibrium at 2500K, [HCl]=0.0625M and [H2]=[Cl2]=0.00450M for the reaction H2+Cl2 ⇌ HCl.
ASHA 777 [7]

Answer:

a. H_2+Cl_2 \rightleftharpoons 2HCl

b. K = 192.9

c. Products are favored.

Explanation:

Hello!

a. In this case, according to the unbalanced chemical reaction we need to balance HCl as shown below:

H_2+Cl_2 \rightleftharpoons 2HCl

In order to reach 2 hydrogen and chlorine atoms at both sides.

b. Here, given the concentrations at equilibrium and the following equilibrium expression, we have:

K=\frac{[HCl]^2}{[H_2][Cl_2]}

Therefore, we plug in the data to obtain:

K=\frac{(0.0625)^2}{(0.00450)(0.00450)}\\\\K=192.9

c. Finally, we infer that since K>>1 the forward reaction towards products is favored.

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Explanation:

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