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Dafna1 [17]
3 years ago
7

Find the empirical and molecular formula for a molar mass of 60.10g/mol; 39.97% carbon 13.41% hydrogen: 46.62% nitrogen

Chemistry
1 answer:
PSYCHO15rus [73]3 years ago
5 0
Assuming we have 100g, this means that

39.97g Carbon * 1 mol / 12 g = 3.33 mol Carbon
13.41g Hydrogen * 1 mol/1 g = 13.41 mol Hydrogen
46.62g Nitrogen * 1 mol / 14 g = 3.33 mol Nitrogen
Dividing everything by 3.33, we get

1 mol Carbon, 4.03 mol Hydrogen, 1 mol Nitrogen.

Empirical formula is CH4N

<span>The mass of the empirical formula is
12 + 4 + 14 = 30

Since the molar mass is double, we multiply all our subscripts

The molecular formula is C2H8N2

The answers to this question are </span><span>an empirical formula of CH4N</span> and a molecular formula of C2H8N2 .
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Answer:

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Number of protons 29

Number of electrons 28

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To get the element symbol, we need the name of the element. To correctly identify the name of the element, we need the proton number.

Now the mass number is 65 and the number of neutrons is 36. The number of protons is this the mass number minus the number of neutrons. This equals 65 - 36 = 29 protons.

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Now to get the number of electrons, for an electrically neutral atom , the number of electrons equals the number of protons. But here, the atom is not electrically neutral anymore as it has now formed a univalent positive ion of +1.

To form a positive ion, you have to do so by losing electrons. The atom in question here has just lost one electron. Thus, our of the 29, it is left with only 28 electrons.

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