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GaryK [48]
3 years ago
7

Un hidrocarburo tiene como composición en masa: C= 85.8% ; H= 14.2% . Como dato nos brindan que una molécula de este compuesto p

esa: LaTeX: 2.1x10^{-22}g2.1 x 10 − 22 g. Hallar la fórmula molecular. Datos: P.A (uma): C=12, H=1
Chemistry
1 answer:
OLga [1]3 years ago
8 0

Answer:

C_{9.042}H_{17.958}

Explanation:

(This exercise has been written in Spanish and for that reason explanation will be held in such language)

Por la definición del Número de Avogadro, un mol del compuesto contiene 6.022 \times 10^{23} moléculas. La masa de un mol se determina mediante regla de tres simple:

x = \frac{6.022\times 10^{23}\,molecules}{1\,molecule} \times (2.1\times 10^{-22}\,g)

x = 126.462\,g

Las participaciones másicas del carbono y el hidrógeno son, respectivamente:

m_{C} = 0.858\cdot (126.462\,g)

m_{C} = 108.504\,g

m_{H} = 126.462\,g - 108.504\,g

m_{H} = 17.958\,g

Ahora, el número de moles de cada elemento es calculado a continuación:

n_{C} = \frac{108.504\,g}{12\,\frac{g}{mol} }

n_{C} = 9.042\,mol

n_{H} = \frac{17.958\,g}{1\,\frac{g}{mol} }

n_{H} = 17.958\,mol

La fórmula molecular del hidrocarburo es:

C_{9.042}H_{17.958}

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bezimeni [28]

<u>Answer:</u> The average atomic mass of X is 28.09 amu

<u>Explanation:</u>

Average atomic mass of an element is defined as the sum of masses of each isotope each multiplied by their natural fractional abundance.

Formula used to calculate average atomic mass follows:

\text{Average atomic mass }=\sum_{i=1}^n\text{(Atomic mass of an isotopes)}_i\times \text{(Fractional abundance})_i .....(1)

  • <u>For isotope 1:</u>

Mass of isotope 1 = 27.979 amu

Percentage abundance of isotope 1 = 92.21 %

Fractional abundance of isotope 1 = 0.9212

  • <u>For isotope 2:</u>

Mass of isotope 2 = 28.976 amu

Percentage abundance of isotope 2 = 4.70 %

Fractional abundance of isotope 2 = 0.0470

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Mass of isotope 3 = 29.974 amu

Percentage abundance of isotope 3 = 3.09 %

Fractional abundance of isotope 3 = 0.0309

Putting values in equation 1, we get:

\text{Average atomic mass of X}=[(27.979\times 0.9212)+(28.976\times 0.0470)+(29.974\times 0.0309)]

\text{Average atomic mass of X}=28.09amu

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3 years ago
If the compound has a molar mass of 156 g/mol, what is its molecular formula?
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I believe that the choices for this question are:
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