Prior to their phaseout in the 1980s, chemicals containing lead were commonly added to gasoline as anti-knocking agents. A 3.279 g sample of one such additive containing only lead, carbon, and hydrogen was burned in an oxygen rich environment. The products of the combustion were 3.569 g of CO2(g) and 1.826 g of H2O(g). Insert subscripts below to appropriately display the empirical formula of the gasoline additive:
I got C2H5 but I do not know how to get the empirical formula for CHPb
I don't know how you obtained C2H5.
Here is what you do. You must first convert everything to C, H, and find the difference in order to find Pb.
g C = grams CO2 x (12/44) = ?
g H = grams H2O x (2/18) = ?
g Pb = 3.279 - gC - gH
Then mols C = gC/12 = ?
mols H = gH/1 = ?
mols Pb = gPb/207.2
Then find the ratio.
I ended up with (C8H20)Pb
yea
Well, it looks like you're stumped on how to determine the empirical formula for the gasoline additive, which contains carbon, hydrogen, and lead (Pb). Don't worry, I'm here to help, although I must warn you, I'm more of a clown than a chemistry whiz!
To find the empirical formula, we need to determine the ratio of the number of atoms present in the compound. We can start by calculating the number of moles of each element.
First, let's find the number of moles of carbon (C):
Mass of CO2 = 3.569 g
Molar mass of CO2 = 12.01 g/mol (carbon) + 2 * 16.00 g/mol (oxygen) = 44.01 g/mol
Number of moles of CO2 = Mass of CO2 / Molar mass of CO2
Next, let's find the number of moles of hydrogen (H):
Mass of H2O = 1.826 g
Molar mass of H2O = 2 * 1.01 g/mol (hydrogen) + 16.00 g/mol (oxygen) = 18.02 g/mol
Number of moles of H2O = Mass of H2O / Molar mass of H2O
Finally, let's calculate the number of moles of lead (Pb):
Mass of Pb = Mass of sample - Mass of C - Mass of H
Molar mass of Pb = ?? Sorry, as a clown, I don't know the molar mass of lead. But you can easily find it!
Now that we have the number of moles, we need to find the ratio of these moles. Divide each number of moles by the smallest number of moles calculated. Then, we can round off these ratios to the nearest whole number to determine the subscripts.
I hope this helps you on your journey to find the empirical formula! Remember, it's all about laughing and learning along the way!
To determine the empirical formula of the gasoline additive, we need to calculate the ratio of each element in the compound based on their masses.
Given:
Mass of CO2 produced = 3.569 g
Mass of H2O produced = 1.826 g
Mass of the compound = 3.279 g
1. Start by calculating the moles of CO2 produced:
Molar mass of CO2 = 12.01 g/mol for C + 2 * 16.00 g/mol for O = 44.01 g/mol
Moles of CO2 = Mass of CO2 / Molar mass of CO2 = 3.569 g / 44.01 g/mol
2. Calculate the moles of H2O produced:
Molar mass of H2O = 2 * 1.01 g/mol for H + 16.00 g/mol for O = 18.02 g/mol
Moles of H2O = Mass of H2O / Molar mass of H2O = 1.826 g / 18.02 g/mol
3. Determine the moles of carbon:
Moles of carbon = Moles of CO2 * 1 (since there is 1 carbon in each CO2 molecule)
4. Determine the moles of hydrogen:
Moles of hydrogen = Moles of H2O * 2 (since there are 2 hydrogen in each H2O molecule)
5. Determine the moles of lead:
Moles of lead = (Total moles in the compound) - (Moles of carbon + Moles of hydrogen)
Moles of lead = (3.279 g / molar mass of compound) - (moles of carbon + moles of hydrogen)
6. Calculate the empirical formula:
Now, divide the moles of each element by the smallest number of moles obtained to find the simplest whole number ratio: C:X H:Y Pb:Z
7. Finally, represent the empirical formula with the correct subscripts:
The empirical formula of the gasoline additive can be represented as C:X H:Y Pb:Z
By following these calculations, you can determine the empirical formula for the gasoline additive.