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15 November, 04:52

8.84 g of a compound is analyzed and found to contain 3.53 g of C, 0.295 g of H, 4.08 g of N, and 0.935 g of O. Which of the following could be the molecular formula for this compound?

C5H10N3O3

1. C10H10N10O2

2. C2H4N6O

3. C8H8N8O4

4. C4H8N6O2

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Answers (1)
  1. 15 November, 05:20
    0
    Option 1 is correct. C10H10N10O2

    Explanation:

    Step 1: Data given

    Mass of a compound = 8.84 grams

    Mass of C = 3.53 grams

    Mass of H = 0.295 grams

    Mass of N = 4.08 grams

    Mass of O = 0.935 grams

    Atomic mass C = 12.01 g/mol

    Atomic mass H = 1.01 g/mol

    Atomic mass N = 14.0 g/mol

    Atomic mass O = 16.0 g/mol

    Step 2: Calculate moles

    Moles = mass / molar mass

    Moles C = 3.53 grams / 12.01 g/mol

    Moles C = 0.294 moles

    Moles H = 0.295 grams / 1.01 g/mol

    Moles H = 0.292 moles

    Moles N = 4.08 grams / 14.0 g/mol

    Moles N = 0.291 moles

    Moles O = 0.935 grams / 16 g/mol

    Moles O = 0.0584 moles

    Step 3: Calculate mol ratio

    We divide by the smallest amount of moles

    C: 0.294 / 0.0584 = 5

    H: 0.292 / 0.0584 = 5

    N: 0.291/0.0584 = 5

    O: 0.0584/0.0584 = 1

    The empirical formula is C5H5N5O

    Option 1 has this empirical formula

    C10H10N10O2
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