molar mass of CO2
C - 12.01 (1) = 12.01
O - 16 (2) = 32
12.01 + 32 = 44.01 g/mol
molar mass of H2O:
H - 1.01 (2) = 2.02
O - 16 (1) = 16
16 + 2.02 = 18.02 g/mol
A compound contains only C, H, and N. Combustion of 35.0 mg of the compound produces 33.5 mg CO2 and 41.1 mg H2O. What is the empirical formula of the compound?
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