Combustion analysis of 1.200 g of an unknown compound containing carbon, hydrogen, and oxygen produced 2.086 g of CO2 and 1.134 g of H2O. What is the empirical formula of the compound?
Added by Marcus J.
Step 1
First, we need to find the moles of carbon and hydrogen in the compound. We can do this by using the moles of CO2 and H2O produced during combustion. 2.086 g CO2 * (1 mol CO2 / 44.01 g CO2) * (1 mol C / 1 mol CO2) = 0.0474 mol C 1.134 g H2O * (1 mol H2O / 18.02 Show more…
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