Complete combustion of 8.80 g of a hydrocarbon produced 26.7 g of CO2 and 13.6 g of H2O. What is the empirical formula for the hydrocarbon?

Question

parthkohli · Answer

$$\rm hydrocarbon + CO_2 \longrightarrow H_2O  + CO_2$$Number of moles of $\rm H_2O = 13.6/18$.  
Number of moles of $\rm H  = 13.6/ 9$.

Number of moles of $\rm CO_2  =  26.7/44$.
Number of moles of $\rm C = 26.7/44$.

The ratio of $\rm H:C$ is $13.6/9 \div 26.7/44 \approx 5:2$.  The empirical formula, thus, seems to be $\rm C_2 H_5$.

koikkara · Answer

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koikkara · Answer

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