The compound known as butylated hydroxytoluene, abbreviated as BHT, contains carbon, hydrogen, and oxygen. A 2.751 g sample of BHT was combusted in an oxygen rich environment to produce 8.241 g of CO2(g) and 2.699 g of H2O(g) .
Insert subscripts to complete the empirical formula of BHT.
BHT + O2 ==> CO2 + H2O
2.751g..............8.241g....2.699 g
I'm rounding all through the calculation and not carrying out to 4 places.
grams C = 8.241 x (12/44) = 2.247
grams H = 2.699 x 2/18 = 0.2999
grams O = 2.751 - 2.247 - 0.2999 = 0.2041
mols C = 2.247/12 = 0.1872
mols H = 0.2999/1 = 0.2999
mols O = 0.2041/16 = 0.01276
To complete, divide all by the smallest.
C = 0.1872/0,01276 = 14.67 rounds to 15
H = 0.2999/0.01276 = 23.503 rounds to 24
O = 0.01276/0.01276 = 1.000
So the empirical formula is C15H24O
The rounding looks even better if I had used molar masses and atomic masses to more than two places.
Well, I must say, this question is really burning with excitement! Let's get down to business and figure out the empirical formula of BHT.
First, let's find the number of moles of CO2 produced. To do that, we divide the mass of CO2 by the molar mass of CO2 (44.01 g/mol):
moles of CO2 = 8.241 g / 44.01 g/mol = 0.1872 mol CO2
Next, let's find the number of moles of H2O produced. We divide the mass of H2O by the molar mass of H2O (18.02 g/mol):
moles of H2O = 2.699 g / 18.02 g/mol = 0.1499 mol H2O
Now, let's find the number of moles of carbon in BHT. From the balanced combustion equation, we know that 1 mole of BHT produces 1 mole of CO2. So, the number of moles of carbon in BHT is the same as the moles of CO2:
moles of carbon = moles of CO2 = 0.1872 mol C
Similarly, the number of moles of hydrogen in BHT is the same as the moles of water:
moles of hydrogen = moles of H2O = 0.1499 mol H
Lastly, the number of moles of oxygen in BHT can be calculated by subtracting the moles of carbon and hydrogen from the total moles of oxygen atoms in CO2 and H2O. Since there are 2 oxygen atoms in CO2 and 1 oxygen atom in H2O, we have:
moles of oxygen = moles of CO2 × 2 + moles of H2O = (0.1872 mol CO2 × 2) + 0.1499 mol H2O = 0.5243 mol O
Now that we have the number of moles of each element, let's find the empirical formula. Dividing the number of moles of each element by the smallest number of moles (in this case, the moles of hydrogen), we get:
carbon: 0.1872 mol / 0.1499 mol ≈ 1.248
hydrogen: 0.1499 mol / 0.1499 mol = 1
oxygen: 0.5243 mol / 0.1499 mol ≈ 3.5
Since we're dealing with whole numbers, let's multiply them by 2 to get a simpler ratio:
carbon: 1.248 × 2 ≈ 2.496, which we can round to 2
hydrogen: 1 × 2 = 2
oxygen: 3.5 × 2 = 7
So, the empirical formula of BHT is C2H2O7.
Wow, that's a mouthful! But don't worry, Clown Bot is here to help with chemistry formulas and jokes too! Let me know if there's anything else I can assist you with!
To determine the empirical formula of BHT, we need to calculate the moles of carbon, hydrogen, and oxygen in the given compounds.
1. Calculate the moles of CO2:
Molar mass of CO2 = 12.01 g/mol + 2(16.00 g/mol) = 44.01 g/mol
Moles of CO2 = mass of CO2 / molar mass of CO2
Moles of CO2 = 8.241 g / 44.01 g/mol = 0.187 moles
2. Calculate the moles of H2O:
Molar mass of H2O = 2(1.01 g/mol) + 16.00 g/mol = 18.02 g/mol
Moles of H2O = mass of H2O / molar mass of H2O
Moles of H2O = 2.699 g / 18.02 g/mol = 0.150 moles
3. Determine the moles of carbon:
Moles of carbon = moles of CO2
Moles of carbon = 0.187 moles
4. Determine the moles of hydrogen:
Moles of hydrogen = 2 x moles of H2O
Moles of hydrogen = 2 x 0.150 moles = 0.300 moles
5. Determine the moles of oxygen:
Moles of oxygen = (mass of BHT - mass of carbon - mass of hydrogen) / molar mass of oxygen
Moles of oxygen = (2.751 g - (0.187 moles x 12.01 g/mol) - (0.300 moles x 1.01 g/mol)) / 16.00 g/mol
Moles of oxygen = 1.049 g / 16.00 g/mol = 0.0656 moles
6. Convert the moles to whole numbers by dividing by the smallest number of moles:
Empirical ratio = moles of carbon : moles of hydrogen : moles of oxygen
Empirical ratio = 0.187 moles : 0.300 moles : 0.0656 moles
Dividing by 0.0656 gives: 2.85 : 4.57 : 1
7. Write the empirical formula:
The subscripts of carbon, hydrogen, and oxygen in the empirical formula of BHT are approximately 3:5:1. Thus, the empirical formula of BHT is C3H5O.
To find the empirical formula of BHT, we need to determine the ratio of carbon, hydrogen, and oxygen atoms in the compound.
First, let's find the number of moles of carbon, hydrogen, and oxygen in the sample.
The molar masses (atomic weights) are as follows:
Carbon (C) = 12.01 g/mol
Hydrogen (H) = 1.008 g/mol
Oxygen (O) = 16.00 g/mol
Moles of CO2 = mass of CO2 / molar mass of CO2
Moles of CO2 = 8.241 g / (12.01 g/mol + 2 * 16.00 g/mol)
Moles of CO2 = 8.241 g / 44.01 g/mol
Moles of CO2 = 0.1871 mol
Moles of H2O = mass of H2O / molar mass of H2O
Moles of H2O = 2.699 g / (2 * 1.008 g/mol + 16.00 g/mol)
Moles of H2O = 2.699 g / 18.02 g/mol
Moles of H2O = 0.1498 mol
Now, let's find the moles of carbon and hydrogen in the empirical formula.
Moles of carbon = moles of CO2
Moles of carbon = 0.1871 mol
Moles of hydrogen = 2 * moles of H2O
Moles of hydrogen = 2 * 0.1498 mol
Moles of hydrogen = 0.2996 mol
The ratio of carbon to hydrogen in the empirical formula will be:
Carbon : Hydrogen = 0.1871 mol : 0.2996 mol
Carbon : Hydrogen = 1 : 1.601
Since we need to have whole numbers, let's multiply both numbers by a factor to make the ratio simple. In this case, we'll use 5.
Carbon : Hydrogen = 5 : 8.005
Therefore, the empirical formula of BHT is C5H8O.