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A 0.539g sample of a compound that contained only carbon and hydrogen was subjected to combustion analysis. The combustion produced 1.64g of carbon dioxide and 0.807 g of water. Calculate the percentage composition and teh empirical formula of the sample.
Steps i took:
1. Find moles.
CO2 -> 0.0373moles, H2O -> 0.0448moles
2. Find mass of C and H:
C: 0.448g, H: 0.0905g
3. Find % composition:
C: 83.3%, H: 16.7%
^ this answer is correct, but...
4. Find Empirical formula:
I assume that there are 100g of sample.
So C will be 83.3g and H will be 16.7g. Then i find the number of moles, which is 6.93 (for C) and 16.5 (for H)... And get the smallest ratio which is 1:2, but the book says it's C5H12. ._.?
Steps i took:
1. Find moles.
CO2 -> 0.0373moles, H2O -> 0.0448moles
2. Find mass of C and H:
C: 0.448g, H: 0.0905g
3. Find % composition:
C: 83.3%, H: 16.7%
^ this answer is correct, but...
4. Find Empirical formula:
I assume that there are 100g of sample.
So C will be 83.3g and H will be 16.7g. Then i find the number of moles, which is 6.93 (for C) and 16.5 (for H)... And get the smallest ratio which is 1:2, but the book says it's C5H12. ._.?
