A 8.408 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 12.53 grams of CO2 and 3.849 grams of H2O are produced.
In a separate experiment, the molar mass is found to be 118.1 g/mol. Determine the empirical formula and the molecular formula of the organic compound.
Find empirical formula and molecular formula.
Put in order of C,H,O.
JILLIAN, Alan. We prefer to keep the same screen name. Refer to your other problem. It a little simpler with just CxHy. This one is CxHyOz. The only difference is this.
Convert 12.53 g CO2 to g C.
Convert 3.849 g H2O to g H.
To find g O, it is
g O = 8.408 g - g C - g H
Then convert g C to mols C, g H to mols H, and g O to mols O.
Then convert these to ratios of whole numbers the same was as the other problem. The molecular formula is done the same way, also.
i literally have no idea how to do these and your explanations are not helping..... like i have no example and i need you to work one out and i can do the other but they are do soon and i have no clue what you are saying.
See my response to your earlier CxHy question below. I've worked it in detail. I hope things work out for you very well.
To determine the empirical formula and molecular formula of the organic compound, we need to follow a series of steps:
Step 1: Calculate the moles of carbon, hydrogen, and oxygen in the sample.
To do this, you need to calculate the moles of carbon dioxide (CO2) and water (H2O) produced during combustion analysis.
The molar mass of CO2 is 44 g/mol, so the moles of CO2 can be calculated as:
moles of CO2 = mass of CO2 / molar mass of CO2
Similarly, the molar mass of H2O is 18 g/mol, so the moles of H2O can be calculated as:
moles of H2O = mass of H2O / molar mass of H2O
Using the given masses of CO2 and H2O, we can substitute the values and calculate the moles of carbon and hydrogen.
moles of CO2 = 12.53 g / 44 g/mol
moles of H2O = 3.849 g / 18 g/mol
Step 2: Determine the moles of carbon, hydrogen, and oxygen in the organic compound.
In the organic compound, CO2 is formed from the carbon component, and H2O is formed from the hydrogen component. The remaining mass of the sample can be attributed to oxygen.
moles of carbon = moles of CO2
moles of hydrogen = (2 * moles of H2O)
moles of oxygen = (mass of sample - (moles of carbon * molar mass of carbon) - (moles of hydrogen * molar mass of hydrogen)) / molar mass of oxygen
Step 3: Find the empirical formula.
The empirical formula represents the simplest whole number ratio of atoms in a compound. To find the empirical formula, divide the moles of each element by the smallest number of moles obtained.
Let's assume the empirical formula has a subscripts of n, so the empirical formula can be written as CnHmOn.
Divide the moles of each element by the smallest number of moles (either carbon, hydrogen, or oxygen) obtained in Step 2.
empirical formula: CnHmOn
Step 4: Calculate the empirical formula mass (EFM).
The empirical formula mass is the sum of the atomic masses of all the atoms in the empirical formula. To calculate the EFM, multiply the number of atoms in each element by the atomic mass of that element.
EFM = (n * atomic mass of carbon) + (m * atomic mass of hydrogen) + (o * atomic mass of oxygen)
Step 5: Calculate the empirical formula molar mass (EFMM).
The empirical formula molar mass is the mass of one mole of the empirical formula.
EFMM = EFM * (1 g/mol)
Step 6: Calculate the empirical formula factor (EFF).
The empirical formula factor is the ratio of the molar mass of the compound to the empirical formula molar mass.
EFF = molar mass of the compound / EFMM
Step 7: Find the whole number ratio of the empirical formula by multiplying all the subscripts (n, m, o) by the empirical formula factor (EFF).
empirical formula ratio: (n * EFF):(m * EFF):(o * EFF)
Step 8: Determine the molecular formula.
The molecular formula represents the actual number of atoms of each element in a molecule. It can be obtained by finding the multiple of the empirical formula ratio that gives a whole number ratio.
Let's assume the molecular formula has subscripts x, y, and z, so the molecular formula can be written as CxHyOz.
Multiply the subscripts in the empirical formula ratio by an integer (x, y, z) that results in a whole number ratio. To determine this integer, divide the given molar mass of the compound by the empirical formula molar mass.
Molecular formula: CxHyOz
That's the step-by-step process to determine the empirical and molecular formulas of the organic compound based on the given information. So, fill in the appropriate values in each step to find the answer.