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3 years ago

What is the empirical formula of a molecule containing 65.5% carbon, 5.5% hydrogen, and 29.0% oxygen?

Chemistry

1 answer:

rusak2 [61]3 years ago

8 0

Answer:

The empirical formula is C3H3O

Explanation:

Step 1: Data given

Suppose the mass of the molecule = 100 grams

The molecule contains:

65.5 % Carbon = 65.5 grams

5.5 % Hydrogen = 5.5 grams

29.0% Oxygen = 29.0 grams

Molar mass of C = 12 g/mol

Molar mass of H = 1.01 g/mol

Molar mass of O = 16 g/mol

Step 2: Calculate moles

Moles = mass / molar mass

Moles C = 65.5 grams / 12 g/mol = 5.46 moles

Moles H = 5.5 / 1.01 g/mol = 5.45 moles

Moles O = 29.0 grams / 16 g/mol = 1.8125 moles

Step 3: Calculate mol ratio

We divide by the smallest amount of moles

C: 5.46 / 1.8125 = 3

H = 5.45 / 1.8125 = 3

O = 1.8125/1.8125 = 1

The empirical formula is C3H3O

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Complete Question

The complete question is shown on the first uploaded image

Answer:

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For Proton Hd, number of non equivalent protons n= 0

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Explanation:

Considering the first question the rule used for prediction of splitting pattern is n+1 (Pascal's Triangle rule), where n is number of H atom on the adjacent carbon which are non equivalent.

According to that for molecule 1 as shown on the second uploaded image

For Proton Ha, number of non equivalent protons n= 2

Splitting pattern for Ha= 2+1 , Triplet

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Splitting pattern for Hb and Hc= 3+1 , Quartet

For Proton Hd, number of non equivalent protons n= 0

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