BHT + O2 ==> CO2 + H2O
2.751g..............8.241g....2.699 g
I'm rounding all through the calculation and not carrying out to 4 places.
grams C = 8.241 x (12/44) = 2.247
grams H = 2.699 x 2/18 = 0.2999
grams O = 2.751 - 2.247 - 0.2999 = 0.2041
mols C = 2.247/12 = 0.1872
mols H = 0.2999/1 = 0.2999
mols O = 0.2041/16 = 0.01276
To complete, divide all by the smallest.
C = 0.1872/0,01276 = 14.67 rounds to 15
H = 0.2999/0.01276 = 23.503 rounds to 24
O = 0.01276/0.01276 = 1.000
So the empirical formula is C15H24O
The rounding looks even better if I had used molar masses and atomic masses to more than two places.
The compound known as butylated hydroxytoluene, abbreviated as BHT, contains carbon, hydrogen, and oxygen. A 2.751 g sample of BHT was combusted in an oxygen rich environment to produce 8.241 g of CO2(g) and 2.699 g of H2O(g) .
Insert subscripts to complete the empirical formula of BHT.
1 answer
1 answer