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neonofarm [45]
3 years ago
8

Vitamin C contains only carbon, hydrogen, and oxygen. When a 1.00 g was combusted, 1.4991 g of CO2 and 0.4092 g of H2O were obta

ined. Determine the empirical formula for this vitamin.
Chemistry
1 answer:
Alina [70]3 years ago
5 0

The empirical formula for this vitamin : C₃H₄O₃

<h3>Further explanation   </h3>

The empirical formula is the smallest comparison of atoms of compound =mole ratio of the components

The principle of determining empirical formula

  • Determine the mass ratio of the constituent elements of the compound.  
  • Determine the mole ratio by dividing the percentage by the atomic mass

Mass of C in CO₂ :(MW C = 12 g/mol, CO₂=44 g/mol)

\tt \dfrac{12}{44}\times 1.4991=0.409~g

Mass of H in H₂O :(MW H = 1 g/mol, H₂O = 18 g/mol)

\tt \dfrac{2.1}{18}\times 0.4092=0.0455~g

Mass O = Mass sample - (mass C + mass H) :

\tt 1-(0.409+0.0455)=0.5455~g

mol ratio C : H : O =

\tt \dfrac{0.409}{12}\div \dfrac{0.0455}{1}\div \dfrac{0.5455}{16}\\\\0.0341\div 0.0455\div 0.0341\rightarrow 1\div 1.33\div 1=3\div 4\div 3

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Answer:

45.3°C

Explanation:

Step 1:

Data obtained from the question.

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Final temperature (T2) =.?

Step 2:

Conversion of celsius temperature to Kelvin temperature.

This is illustrated below:

T(K) = T(°C) + 273

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Initial temperature (T1) = 26°C + 273 = 299K.

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Determination of the new temperature of the gas. This can be obtained as follow:

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Cross multiply to express in linear form

82 x T2 = 299 x 87.3

Divide both side by 82

T2 = (299 x 87.3) /82

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Step 4:

Conversion of 318.3K to celsius temperature. This is illustrated below:

T(°C) = T(K) – 273

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Answer:

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