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An organic compound is 53.1% of carbon, 6.2% Hydrogen, 12.4% nitrogen and 28.3% oxygen by mass . Calculate the molecular formular of the compound if the vapour density is 56.5

Accepted Answer
Step 1: Convert the percentage composition to grams

Assuming 100 g of the compound:

Carbon: 53.1 g
Hydrogen: 6.2 g
Nitrogen: 12.4 g
Oxygen: 28.3 g

Step 2: Convert grams to moles

Carbon: 53.1 g * (1 mol C / 12.01 g/mol) = 4.42 mol C
Hydrogen: 6.2 g * (1 mol H / 1.01 g/mol) = 6.14 mol H
Nitrogen: 12.4 g * (1 mol N / 14.01 g/mol) = 0.885 mol N
Oxygen: 28.3 g * (1 mol O / 16.00 g/mol) = 1.77 mol O

Step 3: Determine the mole ratio

Divide each mole value by the smallest mole value (0.885 mol N):

Carbon: 4.42 mol C / 0.885 mol N = 5
Hydrogen: 6.14 mol H / 0.885 mol N = 7
Nitrogen: 0.885 mol N / 0.885 mol N = 1
Oxygen: 1.77 mol O / 0.885 mol N = 2

Step 4: Multiply the mole ratio by a factor to obtain whole numbers

In this case, multiplying by 5 yields whole numbers:

Carbon: 5 * 5 = 25
Hydrogen: 7 * 5 = 35
Nitrogen: 1 * 5 = 5
Oxygen: 2 * 5 = 10

Therefore, the molecular formula of the compound is C25H35N5O10

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