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3 years ago

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Write the molecular formula for the compound that exhibits a molecular ion at M+ = 112.0499. Assume that C, H, N, and O might be

present, and use the exact masses below: Exact mass of carbon = 12.000 Exact mass of hydrogen = 1.0078 Exact mass of nitrogen = 14.003 Exact mass of oxygen = 15.995 (The order of atoms should be carbon, then hydrogen, then the others in alphabetical order. If there is more than one answer, just give one. ) Molecular formula:

1 answer:

IceJOKER [234]3 years ago

7 0

Answer:

C₅H₈N₂O

Explanation:

The molecular formula denotes the various forms of atoms contained in a molecule at a particular fixed proportion.

The molecular ion M⁺ = 112.0499

and the exact mass values are given as follows:

C = 12.000

H = 1.0078

N = 14.003

O = 15.995

By assumption:

C = 12.000 × 5 = 60.0000

H = 1.0078 × 8 = 1.0078

N = 14.003 × 2 = 28.0060

<u>O = 15.995 × 1 = 15.9950 </u>

<u> = 112.0634 </u>

This is approximtely equal to 112.0499.

As such the Molecular formula for the compound = C₅H₈N₂O

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Moles of ethane gas = $n_2=\frac{18.0 g}{30 g/mol}=0.6 mol$

Moles of propane gas = $n_3$

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$\chi_2=\frac{n_2}{n}=\frac{0.6 mol}{2.22 mol}=0.2703$

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Partial pressure of each gas can be calculated by the help of Dalton's' law:

$p_i=P\times \chi_1$

Partial pressure of methane gas:

$p_1=P\times \chi_1=5.40 atm\times 0.2252=1.22 atm$

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Part B:

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