Problem: A sample of a hydrocarbon is combusted completely in O2(g) to produce 24.01 g CO2(g), 4.917 g H2O(g), and 342 kJ of heat.What is the empirical formula of the hydrocarbon?

FREE Expert Solution

We’re being asked to determine the empirical formula of a compound composed of C and H given the combustion analysis.


We can do a mole-to-mole comparison to determine the mass of C and H.


For C: The molar mass of CO2 is 44.01 g/mol


There is 1 mole of C in 1 mole of CO2. Finding the mass of C:


mass of C=24.01 g CO2×1 mol CO244.01 g CO2×1 mol C1 mol CO2

mass of C = 0.546 mol C


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Problem Details

A sample of a hydrocarbon is combusted completely in O2(g) to produce 24.01 g CO2(g), 4.917 g H2O(g), and 342 kJ of heat.

What is the empirical formula of the hydrocarbon?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Combustion Analysis concept. You can view video lessons to learn Combustion Analysis. Or if you need more Combustion Analysis practice, you can also practice Combustion Analysis practice problems.