A hydrocarbon Y on combustion gives 0.352g of carbon(iv)oxide and 0.18g of water. Calculate the empirical formula of the compound and If the relative molecular mass of Y is 58g, determine the molecular formula of Y.?

...Y + O2 ==> CO2 + H2O

...................0.352 g + 0.18 g
g C in Y is 0.352 x (12/44) = 0.096
g H in Y is 0.18 x (2/18)) = 0.02

mols C in Y = 0.096/12 = 0.008
mols H in Y = 0.02/1 = 0.02
Now find the ratio. The easy way is to divide both numbers by the smallest number; i.e.,
C = 0.008/0.008 = 1
H = 0.02/0.008 = 2.5
Make whole numbers which will be C = 2 and H = 5 so the empirical formula is C2H5. The empirical formula will be (C2H5)x so x is a multiple of the empirical formula. The empirical formula is 29 so 29*what number = 58.
The molecular formula is (C2H5)2 or C4H10. Is the molar mass 59?
4*12 = 48 and 10*1 = 10
48+10 = 58. Bingo.

Well, well, well, hydrocarbons and combustion, huh? Sounds like we're about to light things up with some chemistry!

First, let's calculate the moles of carbon dioxide produced. The molar mass of carbon dioxide is about 44 g/mol. So, moles of carbon dioxide = mass / molar mass = 0.352 g / 44 g/mol = 0.008 mol.

Next, let's calculate the moles of water produced. The molar mass of water is about 18 g/mol. So, moles of water = mass / molar mass = 0.18 g / 18 g/mol = 0.01 mol.

Now, let's determine the moles of carbon and hydrogen in the compound. From the balanced equation for combustion, we know that for each mole of carbon dioxide produced, there is one mole of carbon in the compound, and for each mole of water produced, there is one mole of hydrogen in the compound.

So, moles of carbon = moles of carbon dioxide = 0.008 mol, and moles of hydrogen = moles of water = 0.01 mol.

To determine the empirical formula, we need to find the simplest whole-number ratio of atoms. We'll divide the moles of each element by the smallest number of moles (0.008 mol in this case).

So, the empirical formula is C: 0.008 mol / 0.008 mol = 1, H: 0.01 mol / 0.008 mol = 1.25.

To simplify, we'll multiply both numbers by 4 to get whole numbers: C4H5.

Now, let's determine the molecular formula. We're given that the relative molecular mass (Molar mass) of Y is 58 g/mol, and the empirical formula mass (efm) is approximately 37 g/mol.

To find the molecular formula, we need to divide the relative molecular mass by the empirical formula mass: molecular formula mass / empirical formula mass.

So, 58 g/mol / 37 g/mol = 1.567.

Since we want a whole number, we'll round it down to 1. Now we simply multiply the empirical formula by this number to get the molecular formula.

Molecular formula = C4H5 x 1 = C4H5.

So, the empirical formula of the compound is C4H5, and the molecular formula of Y is also C4H5.

That's chemistry for you! Don't forget to keep those goggles on and stay safe when you're playing with hydrocarbons!

To find the empirical formula of the hydrocarbon Y, we need to find the ratio of carbon to hydrogen in the compound.

1. Start by finding the number of moles of carbon dioxide (CO2) and water (H2O) produced in the combustion reaction:
- Moles of CO2 = Mass of CO2 / Molar mass of CO2
= 0.352 g / (12.01 g/mol + 2 * 16.00 g/mol)
- Moles of H2O = Mass of H2O / Molar mass of H2O
= 0.18 g / (2 * 1.01 g/mol + 16.00 g/mol)

2. Next, determine the mole ratio of carbon to hydrogen in the compound:
- Simplify the mole ratio by dividing both moles of CO2 and H2O by the smaller of the two values obtained.
- This gives you the simplest whole-number ratio of carbon to hydrogen atoms.

3. Finally, determine the empirical formula using the mole ratio obtained in step 2:
- The empirical formula represents the ratio of atoms in the compound in its simplest form, so write the empirical formula using the whole numbers obtained in step 2.

To find the molecular formula of Y, we need to know the relative molecular mass of Y. The relative molecular mass represents the mass of one molecule of Y compared to the mass of one mole of carbon-12 atoms.

1. Calculate the empirical formula mass by summing up the atomic masses of the empirical formula's elements.
- Multiply the atomic mass of each element by the number of atoms in the empirical formula and sum them.

2. Divide the relative molecular mass of Y by the empirical formula mass obtained in step 1.
- This gives you the "n" value, which represents the number of empirical formula units in the molecular formula.

3. Multiply the subscripts of the empirical formula by n to obtain the molecular formula of Y.

By following these steps, you can calculate the empirical formula of the hydrocarbon Y and subsequently determine its molecular formula.

Mega Thanks

C4H10