🤓 Based on our data, we think this question is relevant for Professor Hassell's class at BAYLOR.

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

MM of CO_{2} is 44.01

$\mathrm{mole}\mathrm{of}\mathrm{C}=1.50\overline{)\mathrm{g}{\mathrm{CO}}_{2}}\times \frac{1\overline{)\mathrm{mol}{\mathrm{CO}}_{2}}}{44.01\overline{)\mathrm{g}{\mathrm{CO}}_{2}}}\times \frac{1\mathrm{mol}\mathrm{C}}{1\overline{)\mathrm{mol}{\mathrm{CO}}_{2}}}$

moles of C = 0.034 mol

There are **2 moles of H** in **1 mole of H _{2}O**. Finding the moles of H:

MM of H_{2}O is 18.02

$\mathrm{moles}\mathrm{of}\mathrm{H}=0.766\overline{)\mathrm{g}{\mathrm{H}}_{2}\mathrm{O}}\times \frac{1\overline{)\mathrm{mol}{\mathrm{H}}_{2}\mathrm{O}}}{18.02\overline{)\mathrm{g}{\mathrm{H}}_{2}\mathrm{O}}}\times \frac{2\mathrm{mol}\mathrm{H}}{1\overline{)\mathrm{mol}{\mathrm{H}}_{2}\mathrm{O}}}$

moles of H = 0.085 mol

Upon combustion, a compound containing only carbon and hydrogen produces 1.50 g CO_{2} and 0.766 g H_{2}O. Find the empirical formula of the compound.

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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.

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Based on our data, we think this problem is relevant for Professor Hassell's class at BAYLOR.