Answer:
The empirical formula for the compound is C6H12SO2.
Explanation:
We'll begin by writing out what was given from the question. This is shown:
Let us consider the First experiment:
Mass of the compound = 36.165 mg
Mass of CO2 = 64.425 mg
Mass of H2O = 26.373 mg
Data obtained from the Second experiment:
Mass of compound = 47.029 mg
Mass of SO2 = 20.32 mg
Next, we'll determine the mass of C, H and S. This is illustrated below:
Molar Mass of CO2 = 12 + (2x16) = 44g/mol
Mass of C in CO2 = 12/44 x 64.425 Mass of C = 17.57 mg
Molar Mass of H2O = (2x1) + 16 = 18g/mol
Mass of H in H2O = 2/18 x 26.373
Mass of H = 2.93 mg
Molar Mass of SO2 = 32 + (16x2) = 64g/mol
Mass of S in SO2 = 32/64 x 20.32
Mass of S = 10.16 mg
At this stage, it is important we determine the percentage composition of C, H, S and O. This is illustrated below:
% of C = 17.57/36.165 x 100 = 48.58%
% of H = 2.93/36.165 x 100 = 8.10%
% of S = 10.16/47.029 x 100 = 21.60%
% of O = 100 - (48.58 + 8.1 + 21.6)
% of O = 21.72%
Now we can easily obtain the empirical formula for the compound by doing the following.
Step 1:
Divide by their molar mass
C = 48.58/12 = 4.0483
H = 8.10/1 = 8.1
S = 21.60/32 = 0.675
O = 21.72/16 = 1.3575
Step 2:
Divide by the smallest:
C = 4.0483/0.675 = 6
H = 8.1/0.675 = 12
S = 0.675/0.675 = 1
O = 1.3575/0.675 = 2
From the calculations made above, empirical formula for the compound is C6H12SO2
