what is the empirical formula of a compound composed of 3.25% hydrogen, 19.36% carbon, and 77.39% oxygen? by mass
Need to use the molar weights and assume there is 100g, just to make it easy. 3.25 g of Hydrogen (1 mole H / 1.008 g H) = 3.22 19.36 g of C (1 mole C / 12.01 g C) = 1.61 77.39 g of O (1 mole O / ...
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User: what is the empirical formula of a compound composed of 3.25% hydrogen, 19.36% carbon, and 77.39% oxygen? by mass

Weegy: Need to use the molar weights and assume there is 100g, just to make it easy. 3.25 g of Hydrogen (1 mole H / 1.008 g H) = 3.22 19.36 g of C (1 mole C / 12.01 g C) = 1.61 77.39 g of O (1 mole O / 15.9994 g O) = 4.84 Take the smallest number calculated and divide the others by it. In this case, the smallest was 1.61. So, 1.61/1.61 = 1 . . . So, C = 1. 3.22/1.61 = 2 . . . So, H = 2 4.84/1.61 = 3 . . . So, O = 3 This empirical formula is then: CH2O3

Weegy: what is the empirical formula of a compound composed of 3.25% hydrogen, 19.36% carbon, and 77.39% oxygen by mass?

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