The molecular formula for this compound (14.37% H, density of 1.13 g/L at 24 C and 743 mmHg) is C_H_
I am not sure how to use this information
Determine the empirical formula from the percent composition. The problem should have said it was a hydrocarbon; otherise we don't know the percent carbon. I will assume a hydrocarbon; therefore, %C = 100-%H. Take 100 g sample, then convert each to mols.
14.37/1 = 14.37 mols
85.6%/12 = 7.13
You can tell the ratio is CH2 and that is the empirical formula.
Now you need the molar mass which you can get from
P*molar mass = density*R*T
Solve for molar mass and determine frm that how many of the CH2 units are strung together to make up a mole.
Post your work if you get stuck.
Thank you, that was awesome, I think i got the right answer now
C2H4 is the molecular formula
To determine the molecular formula of the compound, we can use the given information about the percent composition of hydrogen (H) and the density of the compound.
1. Determine the number of moles of hydrogen (H):
- Assume we have 100 g of the compound.
- Since the compound is 14.37% hydrogen, we have 14.37 g of hydrogen.
- To convert grams to moles, divide by the molar mass of hydrogen (1 g/mol).
- So, we have 14.37 g / 1 g/mol = 14.37 mol of hydrogen.
2. Calculate the molar volume of the compound:
- Molar volume is the volume occupied by one mole of a substance.
- We are given the density of the compound, which is 1.13 g/L.
- Convert the density to grams per milliliter (g/mL) since 1 mL = 1 cm³:
- 1.13 g/mL = 1.13 g/cm³
- Convert grams to moles using the molar mass of the compound.
3. Determine the molar mass of the compound:
- Calculate the molar mass by dividing the mass of the compound by the number of moles:
- Molar mass (g/mol) = Mass (g) / Moles (mol)
4. Find the empirical formula:
- The empirical formula shows the simplest whole number ratio of atoms in a compound.
- Convert the moles of each element to the simplest whole number ratio by dividing them by the smallest mole value.
5. Determine the molecular formula:
- The molecular formula is the actual number of atoms of each element in a molecule of the compound.
- To find the molecular formula, we need additional information, such as the molar mass of the compound or its empirical formula.
Unfortunately, without additional information about the molar mass or empirical formula, we cannot determine the molecular formula of the compound.