A compound has an empirical formula, C2H2O. If the experimental molecular weight is found to be in the range of 160-170, the molecular formula of this compound is: (Atomic weight: C = 12.1, H = 1, O = 16).
Correct answer: C. C8H8O4
- A. C3H6O3
- B. C4H4O2
- C. C8H8O4
- D. C6H6O3
Explanation
The molecular mass of the empirical formula is 2(12.1) + 2(1) + 16 = 42.2Now, we need to find 'n' Experimental molecular weight = 165 (average of the given range of 160-170)We can find n byn= (experimental molecular weight) / (empirical formula mass) = 165/42.2 = 3.9 Hence, 'n' is approximately 4 Now, 4C2* 4H2* O4 = C8H8O4 Hence, option C is the correct option.
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