Answer first question :
Assume we have 100 g of the compound.
Then we have 40.00 g of C, 6.67g of H, and 53.33g of O.
Moles of C = 40.00 g C × 1mol C/12.01g C = 3.331 mol C
Moles of H = 6.72 g H × 1 mol H/1.008g H = 6.67 mol H
Moles of O = 53.28 g O × 1 mol O/16.00g O = 3.330 mol H
Moles of C:Moles of H:Moles of O = 3.331:6.67:3.330=1.000:2.00:1 ≈ 1:2:1
The empirical formula is CH₂O.
The empirical formula is the simplest formula of a compound. The actual formula is an integral multiple of the empirical formula.
If the empirical formula is CH₂O, the actual formula is (CH₂O)n or CnH2nOn, where n = 1, 2, 3, … Our job is to determine the value of n.
The empirical formula mass of CH₂O is 30.03 u. The molecular mass of 180.18 u must be some multiple of this number.
for finding the molecular formula
So 55.0⋅g⋅mol−1=n×(12.01+2×1.008+16.00)g⋅mol−1.
n =1.896 ≈ 2
n=2 and the molecular formula is 2×(CH2O) = C2H4O2.
so molecular mass is 60 g/mol
02. (20 POINTS) An unknown substance is empirically determined to be 40 percent carbon by weight,...
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