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2 years ago

The skeletal structure of Arachidonic acid, an essential fatty acid, is provided below. Arachidonic acid is best classified as:

Chemistry

1 answer:

Alexandra [31]2 years ago

4 0

Skeletal structure is missing, so i have attached it.

Answer:

Option B: Omega 6 fatty acid

Explanation:

Arachidonic Acid is defined as an essential and unsaturated fatty acid. It's usually found in animal and human fat including the liver, brain, and also glandular organs. While in animals, it is a constituent of their phosphatides.

Arachidonic Acid is formed as a result of the synthesis from dietary linoleic acid and it's a preliminary stage in the biosynthesis of prostaglandins, thromboxanes, and leukotrienes.

In short, Arachidonic acid is basically a long-chain fatty acid which is a C20, Omega 6 polyunsaturated fatty acid that has four Z-double bonds.

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How is the mass in grams of the element converted to amount in atoms

Alik [6]

A substance's molar mass is calculated by multiplying its relative atomic mass by the molar mass constant (1 g/mol). ... By multiplying a given mass by the molar mass, the amount of moles of the substance can be calculated.

8 0

2 years ago

The molarity of a sodium hydroxide (NaOH) solution is 0.2 M. The molar mass of NaOH is 40 g/mol. If the solution contains 20 g o

mote1985 [20]

Answer:

$\large \boxed{\text{2.5 L}}$

Explanation:

1. Calculate the moles of NaOH.

$\text{Moles} = \text{20 g} \times \dfrac{\text{1 mol}}{\text{40 g}} = \text{0.50 mol}$

2. Calculate the volume of NaOH

$\begin{array}{rcl}\\\text{Molar concentration} &= &\dfrac{\text{moles}}{\text{litres}}\\\\ n &= &\dfrac{c}{V}\\\\\dfrac{\text{0.2 mol}}{\text{1 L}} &=& \dfrac{\text{0.50 mol}}{V}\\\\ \dfrac{0.2V}{\text{1 L}} & = & 0.50\\\\0.2V &= & \text{0.50 L}\\V & = & \dfrac{\text{0.50 L}}{0.2}\\\\& = & \textbf{2.5 L}\\\end{array}\\\text{The volume of the solution is $\large \boxed{\textbf{2.5 L}}$}$

7 0

3 years ago

Read 2 more answers

What are the ionic bonds

zhuklara [117]

Explanation:

Ionic bonds are bonds formed as a result of the electrostatic attraction between two species.

This bond type is an interatomic bond.
It forms when two specie with a large electronegative difference between them combines.
This is usually a metal and a non-metal.
The metal loses its valence electrons and becomes positively charged.
The non-metal gains the electron and becomes negatively charged.
An electrostatic attraction between the two specie leads to the formation of an ionic bond.
They are solids with a high melting point.
They are soluble in polar solvents.

learn more:

Ionic bonds brainly.com/question/6071838

#learnwithBrainly

3 0

2 years ago

What is the [H+] of a solution with a pH of 9.40?

LiRa [457]

Answer:

a) 3.98 x 10^-10

Explanation:

Hello,

In this case, for the given pH, we can compute the concentration of hydronium by using the following formula:

$pH=-log([H^+])$

Hence, solving for the concentration of hydronium:

$[H^+]=10^{-pH}=10^{-9.40}\\$

$[H^+]=3.98x10^{-10}M$

Therefore, answer is a) 3.98 x 10^-10

Best regards.

4 0

3 years ago

A piece of unknown metal weighs 348g. When the metal piece absorbs 6.64kj of heat , its temperature increases from 24.4C to 43.6

Morgarella [4.7K]

Answer:

This metal could be the aluminium with a specific heat of $H = 993 \frac{J}{kgC}$

Explanation:

A pie of unknown metal presents a mass (M) of 348 g. This metal is heated using energy (E) of 6.64 kJ and the temperature increases from T1 =24.4 to T2 =43.6°C. We can calculate the specific heat (H) of this metal as follows

$H = \frac{E}{M*(T2-T1)}$

We can replace previously presented data in this equation. After simplifying and converting to adequated units, we found that

$H = \frac{6640 J}{0.348 Kg*(43.6-24.4) C} =\frac{6640 J}{6.686 KgC}$

Finally, the specific heat of this metal is

$H = 993 \frac{J}{kgC}$

The aluminium could be the metal, its specific heat is similar to that found in this problem.

Finally, we can conclude that this metal could be the aluminium with a specific heat of $H = 993 \frac{J}{kgC}$

7 0

3 years ago