View the step-by-step solution to:

# What is the empirical formula of a compound containing C, H, and O if combustion of 1.23 g of the compound yields 1.8 g CO2 and 0.

What is the empirical formula of a compound containing C, H, and O if combustion of 1.23 g of the compound yields 1.8 g CO2 and 0.74 g H2O

The empirical... View the full answer

Let me explain the... View the full answer

Let me explain the... View the full answer

• moles of C present = 0.49gC/12.01g =0.041 mol C ; moles of H present = 0.083g H/ 1.008gH= 0.082 mols ; moles of O present = 0.657gO/16.00gO = 0.041 moles ; therefore we find the ratio of C, H and O present in the compound by dividing each moles by the smallest number of the moles in this case, 0.041 is the smallest and therefore the ratio is = 1 : 2 : 1 respectively ; therefore the empirical formula of the compound is CH2O.
• okiyaiomuse
• May 06, 2018 at 6:20am
• am sorry i posted the answer by mistake when it was incomplete.....
• okiyaiomuse
• May 06, 2018 at 6:22am

### Why Join Course Hero?

Course Hero has all the homework and study help you need to succeed! We’ve got course-specific notes, study guides, and practice tests along with expert tutors.

### -

Educational Resources
• ### -

Study Documents

Find the best study resources around, tagged to your specific courses. Share your own to gain free Course Hero access.

Browse Documents