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 CO_{2} is** ****44.01 g/mol**

There is **1 mole of C** in **1 mole of CO _{2}**. Finding the mass of C:

$\mathrm{mass}\mathrm{of}\mathrm{C}=24.01\overline{)\mathrm{g}{\mathrm{CO}}_{2}}\times \frac{1\overline{)\mathrm{mol}{\mathrm{CO}}_{2}}}{44.01\overline{)\mathrm{g}{\mathrm{CO}}_{2}}}\times \frac{1\mathrm{mol}\mathrm{C}}{1\overline{)\mathrm{mol}{\mathrm{CO}}_{2}}}$

mass of C = 0.546 mol C

A sample of a hydrocarbon is combusted completely in O_{2}(g) to produce 24.01 g CO_{2}(g), 4.917 g H_{2}O(g), and 342 kJ of heat.

What is the empirical formula of the hydrocarbon?

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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.