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2 March, 00:19

If a compound has a molar mass of 180 g/mol and its empirical formula is CH20, what is its molecular formula?

CH20

C2H402

O C6H1206

C12H22011

+4
Answers (1)
  1. 2 March, 00:47
    0
    C6H12O6

    Explanation:

    The empirical formula is CH2O

    The molecular formula is n times the empirical formula CH2O. With n = 1,2,3, ...

    n = the ratio between molar mass / mass of the empirical formula

    The empirical formula CH2O has:

    C ⇒ 12g/mole

    H2 ⇒ 2*1g/mole = 2g/mole

    O = 16g/mole

    12+2+16 : 30g/mole

    Molar mass of the compound = 180g/mole

    ⇒n = ratio between molar mass / mass of the empirical formula

    n = 180/30 = 6

    This means we have to multiply each element by 6

    6C

    12H

    6O

    The molecular formula is C6H12O6

    If we control this: 6*12 + 12*1 + 6*16 = 72+12+96 = 180g/mole

    This compound is probably glucose (or fructose)
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