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Vinil7 [7]
3 years ago
15

A sample of a compound contains 60.0 g C and 5.05 g H. It’s molar mass is 78.12 g/mol. What is the compound’s molecular formula?

Chemistry
1 answer:
Natalka [10]3 years ago
5 0

Answer:

C6H6

Explanation:

C :     60.0 g*1 mol/12 .01g = 5.00 mol

H:      5.05 g * 1 mol/1.01 g= 5.10 mol

C:H = 5.00 mol : 5.10 mol = 1:1

CH is an empirical formula

Molar mass (12.01 +1.01)=13.02 g/mol

78.12g/mol /13.02 g/mol =6

Molecular formula is the empirical that was taken 6 times (CH)6 = C6H6

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I can't draw diagrams on this web site but I can do with numbers I think. So an electron is moved from n = 1 to n = 5. I'm assuming I've interpreted the problem correctly; if not you will need to make a correction. I'm assuming that you know the electron in the n = 1 state is the ground state so the 4th exited state moves it to the n = 5 level.

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An unknown compound with a molar mass of 223.94 g/mol consists of 32.18% c, 4.50% h, and 63.32% cl. find the molecular formula f
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The actual number of atoms of each element present in the molecule of the compound is represented by the formula known as molecular formula.

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Mass of each element present in the unknown compound is determined as:

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Now, the number of each element in the unknown compound is determined by the formula:

number of moles = \frac{given mass}{molar mass}

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number of moles = \frac{72.06}{12} = 6.005 mole\simeq 6 mole

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Multiplying with 2 to convert the numbers in formula into a whole number:

So, the empirical formula is C_{3}H_{5}Cl_{2}.

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In order to determine the molecular formula:

n = \frac{molar mass}{empirical mass}

n = \frac{223.94}{112} = 1.99 \simeq 2

So, the molecular formula is:

2\times C_{3}H_{5}Cl_{2} =  C_{6}H_{10}Cl_{4}

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