4.760 g of a substance (containing only C, H, and O) is burned in a combustion analysis apparatus.
The mass of CO2 produced is 1.276×101 g, and the mass of H2O produced is 3.134 g.
What is the empirical formula of the compound?
I keep getting CH5O2, which is incorrect!
Why not show your work and let me find the error instead of showing you how to do it.
To determine the empirical formula of a compound from the given information, we need to find the simplest, whole-number ratio of atoms. Here's how to calculate it:
1. Start by finding the moles of carbon and hydrogen in the given data.
- Moles of carbon in CO2 = mass of CO2 / molar mass of CO2
- Molar mass of CO2 = molar mass of C + 2 * molar mass of O
- Molar mass of C = 12.01 g/mol
- Molar mass of O = 16.00 g/mol
So, moles of carbon = (mass of CO2 / molar mass of CO2) = (1.276×10^1 g / (12.01 g/mol + 2 * 16.00 g/mol))
Similarly, moles of hydrogen = (mass of H2O / molar mass of H2O)
2. Now, find the moles of oxygen.
- Moles of oxygen = Total moles of carbon and hydrogen - (moles of carbon + moles of hydrogen)
- The total moles of carbon and hydrogen can be found by dividing the given mass of the substance (4.760 g) by its molar mass.
3. After determining the moles of each element, divide each mole value by the smallest mole value obtained to obtain a whole-number ratio.
4. Finally, use the obtained whole-number ratio to write the empirical formula of the compound.
Performing the calculations, the empirical formula should be calculated as follows:
1. Moles of carbon:
Mass of CO2 = 1.276×10^1 g
Molar mass of CO2 = 12.01 g/mol + 2 * 16.00 g/mol
Moles of carbon = (1.276×10^1 g) / (12.01 g/mol + 2 * 16.00 g/mol)
2. Moles of hydrogen:
Mass of H2O = 3.134 g
Molar mass of H2O = 2 * 1.01 g/mol + 16.00 g/mol
Moles of hydrogen = (3.134 g) / (2 * 1.01 g/mol + 16.00 g/mol)
3. Moles of oxygen:
Total moles of carbon and hydrogen = 4.760 g / molar mass of the compound
Moles of oxygen = Total moles of carbon and hydrogen - (moles of carbon + moles of hydrogen)
4. Divide each mole value by the smallest mole value obtained and round to the nearest whole number if necessary.
5. Use the obtained whole-number ratio to write the empirical formula of the compound.
By correctly following these steps, you will be able to determine the empirical formula of the compound.