A pure organic compound weighing 947.4mg was heated in a stream of oxygen. The effluent gas was swept successively through a tube of magnesium perchlorate dessicant weighing 18.6137g and a tube of Ascarite weighing 16.8425g. After several minutes the tubes were sealed and reweighed. The tube containing the magnesium perchlorate weighed 18.6448g and the tube containing the Ascarite weighed 16.9098g.

Question

Calculate the % H and % C in the sample.
If the compound consisted only of C and H, calculate its empirical formula.

Answer 1

Difference between initial and final weight perchlorate = mass H2O
Difference between initial and final weight ascarite = mass CO2

%H = [(mass H2O x 2*atomic mass H/molar mass H2O)/mass original sample]*100 = ?

% C = [(mass CO2 x atomic mass C/molar mass CO2)/mass original sample]*100 = ?

To find the empirical formula, take 100 g sample which gives the percent C and H in grams.
Convert to mols
Find the ratio of C to H with the smallest number being no less than
1.00. Post your work if you get stuck.

Answer 2

Difference between initial and final perchlorate(18.6137-18.6448) = 0.0311
ascarite(16.8425-16.9098)= 0.0673

%H= (0.0311x2x1.00784/44.00766)/947.4×100= 0.000150355
%C=(0.0673x12.0096/44.0076)/947.4x100=0.001938572

0.000150355x1mol/1.00784= 0.000148866
0.001938572x1mol/12.01= 0.000161413

0.000148866÷0.000148866= 1
0.000161413÷0.000148866=1.08

1×2= 2
1.08×2= 2.17

C2H2 empirical formula

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