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Alex777 [14]
3 years ago
5

La is element 57 on the periodic table a sample contains 2.82 * 10€25 power atoms of La calculate the amount of LA

Chemistry
1 answer:
vodka [1.7K]3 years ago
5 0

Answer:

n=46.8molLa\\\\m=6.50x10^3gLa

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to calculate both moles and grams of lanthanum by using the Avogadro's number as a relationship of atoms to moles and its atomic mass as a relationship to moles to grams to obtain the following:

n=2.82x10^{25}atomsLa*\frac{1molLa}{6.022x10^{23}atomsLa}=46.8molLa\\\\m=46.8molLa*\frac{138.9gLa}{1molLa}  =6.50x10^3gLa

Regards!

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Could someone explain how they got this answer, explain step by step plz
gulaghasi [49]

Answer:

6.018 amu

Explanation:

Let 6–Li be isotope A.

Let 7–Li be isotope B.

Let the abundance of 6–Li be A%

Let the abundance of 7–Li be B%

The following data were obtained from the question:

Atomic mass of isotope A (6–Li) =.?

Atomic mass of isotope B (7–Li ) = 7.015 amu.

Abundance of 7–Li (B%) = 92.58%

Abundance of 6–Li (A%) = 100 – B% = 100 – 92.58 = 7.42%

Atomic mass of Lithium = 6.941amu

The atomic mass of isotope A (6–Li) can be obtained as follow:

Atomic mass = [(Mass of A x A%)/100] + [(Mass of B x B%)/100]

6.941 = [(mass of A x 7.42)/100] + [(7.015x92.58)/100]

6.941 = [(mass of A x 7.42)/100] + 6.494487

(mass of A x 7.42)/100 = 6.941 – 6.494487

(mass of A x 7.42)/100 = 0.446513

Mass of A x 7.42 = 100 x 0.446513

Mass of A x 7.42 = 44.6513

Divide both side by 7.42

Mass of A = 44.6513 / 7.42

Mass of A = 6.018 amu

Therefore, the mass of 6–Li is 6.018 amu

7 0
3 years ago
If the pressure in the room is 759.2 torr and the vapor pressure of water is 23.8 torr, what is the pressure of hydrogen gas in
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The partial pressure of Hydrogen gas can directly be calculated by simply taking the difference of the overall pressure and the vapour pressure of water. That is:

 

P (H2 gas) = 759.2 torr – 23.8 torr

<span>P (H2 gas) = 735.4 torr</span>

6 0
3 years ago
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They’ll have moved the farthest, since the solvent is best at carrying those kinds of materials.
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2 years ago
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Determine the number of grams of sodium carbonate needed to prepare 100.0 ml of a 2.5 m solution
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Answer:

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Explanation:

First we convert 100.0 mL to L:

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Now we <u>calculate how many moles of sodium carbonate are needed</u>, using the <em>definition of molarity</em>:

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  • moles = molarity * liters
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Finally we <u>convert 0.25 moles of sodium carbonate into grams</u>, using its <em>molar mass</em>:

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