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Anettt [7]
3 years ago
8

A compound containing 74.0% carbon, 8.7% hydrogen and 17.3% nitrogen. Determine the

Chemistry
1 answer:
BabaBlast [244]3 years ago
5 0

Answer:

The empirical formula is C5H7N ; the molecular formula is C10H14N2

Explanation:

in 100% compound we have <u>74.0 % Carbon</u> ( Molar mass = 12g/mole), <u>8.7% hydrogen</u> ( Molar mass = 1.01 g/mole) and <u>17.3% Nitrogen</u> (Molar mass = 14.01 g/mole).

Carbon: 74g / 12 = 6.1667

Hydrogen: 8.7/ 1 = 8.7

Nitrogen: 17.3/ 14. = 1.236

⇒1.236 is the smallest so we divide everything through by 1.236

C: 6.1667 / 1.236 =  4.99 ≈ 5

H: 8.7 /1.236 = 7

N: 1.236 / 1.236 = 1

The empirical formula = C5H7N

To find the molecular formula, calculate the molar mass of the empirical formula first.

C= 12g/mole

H=1g/mole

N=14g/ mole

5*12 + 7*1 + 14 = 81

In this case, 81 g/mol. Compare this to the molar mass given in the problem (162 g/mol). The molecular molar mass is <u>twice</u> the empirical molar mass (162/81 = 2), so the subscripts for the molecular formula should be t<u>wice that of the empirical formula </u>

<u />

The molecular formula = C10H14N2 ( which is Nicotine)

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